(a) Interpretation: The direction of the reversible reaction between ATP and creatine is to be stated. Concept introduction: A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by Δ G ° .

Question

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Answer 1

Question

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.

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Students have asked these similar questions

A3

Breakdown rxn of GIUCOSE. What is the Cleland diagram for the reaction glyceraldehyde 3-phosphate to 1,3 diphosphoglycerate? Based this on the following steps: a. Glyceraldehyde3-phosphate binds to the enzyme,E b. NAD binds to the enzyme E then is reduced to NADH c. NADH leaves the enzyme d. Phosphate binds to the enzyme and attacks the glycerate phosphate attached to the enzyme e. 1,3-disphosphoglycerate leaves the enzyme as the final procut

Match with the given reactionA. The reaction that is slowest in reacting with the enzymeB. The reaction that is fastest in reacting with the glucose oxidaseC. The reaction that is most fitted in the active site of the enzyme

Answer 2

Question

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.

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Answer 3

Question

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.

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Answer 4

Question

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.

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Answer 5

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.

Answer 6

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Answer 7

Chapter 15, Problem 12P

Interpretation Introduction

(a)

Interpretation:

The direction of the reversible reaction between ATP and creatine is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Answer 8

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and creatine moves towards the left side of the reaction.

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

The given reversible reaction is given below.

ATP+creatine⇌creatine phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of creatine to creatine phosphate is ΔG°'=−10.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for creatine to creatine phosphateΔG°'=7.3 kcal mol−1−10.3 kcal mol−1=−3 kcal mol−1

Thus, the value of the Gibbs free energy is −3 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Answer 13

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Answer 14

Interpretation Introduction

(b)

Interpretation:

The direction of the reversible reaction between ATP and glycerol is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Answer 15

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glycerol moves towards the right side of the reaction.

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

The given reversible reaction is given below.

ATP+glycerol⇌glycerol 3−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glycerol to glycerol 3-phosphate is ΔG°'=−2.2 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glycerol to glycerol 3−phosphateΔG°'=7.3 kcal mol−1−2.2 kcal mol−1=5.1 kcal mol−1

Thus, the value of the Gibbs free energy is 5.1 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right hand side.

Answer 20

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Answer 21

Interpretation Introduction

(c)

Interpretation:

The direction of the reversible reaction between ATP and pyruvate is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Answer 22

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and pyruvate moves towards the left side of the reaction.

Answer 23

Expert Solution

Answer 24

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

The given reversible reaction is given below.

ATP+pyruvate⇌phosphoenolpyruvate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of pyruvate to phosphoenolpyruvate is ΔG°'=−14.8 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for pyruvate to phosphoenolpyruvateΔG°'=7.3 kcal mol−1−14.8 kcal mol−1=−7.5 kcal mol−1

Thus, the value of the Gibbs free energy is −7.5 kcal mol−1. The negative value of Gibbs free energy indicates that reaction moves in the left hand side.

Answer 27

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.

Answer 28

Interpretation Introduction

(d)

Interpretation:

The direction of the reversible reaction between ATP and glucose is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Answer 29

Expert Solution

Answer to Problem 12P

The reversible reaction between ATP and glucose moves towards the right side of the reaction.

Answer 30

Expert Solution

Answer 31

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

The given reversible reaction is given below.

ATP+glucose⇌glucose 6−phosphate+ADP.

The standard Gibbs free energy for the conversion of ATP to ADP is ΔG°'=−7.3 kcal mol−1.

The given standard Gibbs free energy for the conversion of glucose to glucose6-phosphate is ΔG°'=−3.3 kcal mol−1.

Thus, the change in the standard Gibbs free energy for the conversions is calculated as follows.

Change in ΔG°'= ΔG°' for ATP to ADP− ΔG°' for glucose to glucose 6−phosphateΔG°'=7.3 kcal mol−1−3.3 kcal mol−1=4 kcal mol−1

Thus, the value of the Gibbs free energy is 4 kcal mol−1. The positive value of Gibbs free energy indicates that reaction moves in the right-hand side.