ORGANIC CHEMISRTY(LL)W/CONNECT
5th Edition
ISBN: 9781260100228
Author: SMITH
Publisher: MCG
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Chapter 6, Problem 6.12P
The equilibrium constant for the conversion of the axial to the equatorial conformation of methoxycyclohexane is
a. Given these data, which conformation is present in the larger amount at equilibrium?
b. Is
c. From the values in Table
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The equilibrium constant for the conversion of the axial to the equatorial conformation of methoxycyclohexane is 2.7.
a.) Given these data, which conformation is present in the larger amount at equilibrium?b.) Is ΔGo for this process positive or negative?c.) find the approximate the size of ΔGo.
a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose:
Given ΔG°C6H12O6(s) = -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l)
b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is:
ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole.
c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?
For every two QH2 (ubiquinol) that enter the Q cycle, one is regenerated and the other passes its two electrons to two cytochrome c1 centers. The overall equation is:QH2 + 2 cyt c1 (Fe3+) + 2 H+ → Q + 2 cyt c1 (Fe2+) + 4 H+Calculate the free energy change associated with the Q cycle. Use 3 significant figures.
ΔG°ʹ = ? kJ · mol−1
Chapter 6 Solutions
ORGANIC CHEMISRTY(LL)W/CONNECT
Ch. 6 - Problem 6.1 Classify each transformation as...Ch. 6 - Prob. 6.2PCh. 6 - Problem 6.3 By taking into account...Ch. 6 - Problem 6.4 Use curved arrows to show the movement...Ch. 6 - Problem 6.5 Follow the curved arrows and draw the...Ch. 6 - Prob. 6.6PCh. 6 - Problem 6.7 Use the values in Table 6.2 to...Ch. 6 - Prob. 6.8PCh. 6 - aWhich Keq corresponds to a negative value of G,...Ch. 6 - Given each of the following values, is the...
Ch. 6 - Given each of the following values, is the...Ch. 6 - The equilibrium constant for the conversion of the...Ch. 6 - Prob. 6.13PCh. 6 - For a reaction with H=40kJ/mol, decide which of...Ch. 6 - For a reaction with H=20kJ/mol, decide which of...Ch. 6 - Draw an energy diagram for a reaction in which the...Ch. 6 - Prob. 6.17PCh. 6 - Prob. 6.18PCh. 6 - Problem 6.19 Consider the following energy...Ch. 6 - Draw an energy diagram for a two-step reaction,...Ch. 6 - Which value if any corresponds to a faster...Ch. 6 - Prob. 6.22PCh. 6 - Problem 6.23 For each rate equation, what effect...Ch. 6 - Prob. 6.24PCh. 6 - Identify the catalyst in each equation. a....Ch. 6 - Draw the products of homolysis or heterolysis of...Ch. 6 - Explain why the bond dissociation energy for bond...Ch. 6 - Classify each transformation as substitution,...Ch. 6 - Prob. 6.29PCh. 6 - 6.30 Draw the products of each reaction by...Ch. 6 - 6.31 (a) Add curved arrows for each step to show...Ch. 6 - Prob. 6.32PCh. 6 - Prob. 6.33PCh. 6 - Prob. 6.34PCh. 6 - Calculate H for each reaction. a HO+CH4CH3+H2O b...Ch. 6 - Homolysis of the indicated CH bond in propene...Ch. 6 - Prob. 6.37PCh. 6 - Prob. 6.38PCh. 6 - 6.39. a. Which value corresponds to a negative...Ch. 6 - Prob. 6.40PCh. 6 - For which of the following reaction is S a...Ch. 6 - Prob. 6.42PCh. 6 - Prob. 6.43PCh. 6 - 6.44 Consider the following reaction: .
Use curved...Ch. 6 - Prob. 6.45PCh. 6 - Draw an energy diagram for the Bronsted-Lowry...Ch. 6 - Prob. 6.47PCh. 6 - Indicate which factors affect the rate of a...Ch. 6 - Prob. 6.49PCh. 6 - 6.50 The conversion of acetyl chloride to methyl...Ch. 6 - Prob. 6.51PCh. 6 - Prob. 6.52PCh. 6 - The conversion of (CH3)3Cl to (CH3)2C=CH2 can...Ch. 6 - 6.54 Explain why is more acidic than , even...Ch. 6 - Prob. 6.55PCh. 6 - Prob. 6.56PCh. 6 - Prob. 6.57PCh. 6 - Although Keq of equation 1 in problem 6.57 does...Ch. 6 - Prob. 6.59P
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- In glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be present as described by the following equation:Glu+ATP⟶G6P+ADP ΔG°=−17 kJ In this process, ATP becomes ADP summarized by the following equation:ATP⟶ADP ΔG°=−30 kJ Determine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:Glu⟶G6P ΔG°=?arrow_forwardIn glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be present as described by the following equation:Glu + ATP⟶G6P + ADP ΔG°298 = −17 kJIn this process, ATP becomes ADP summarized by the following equation:ATP⟶ADP ΔG°298 = −30 kJDetermine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:Glu⟶G6P ΔG°298 = ?arrow_forwardDouble-helix-formation entropy. For double-helix forma- tion, DG can be measured to be 254 kJ mol?1 (213 kcal mol?1) at pH 7.0 in 1 M NaCl at 258C (298 K). The heat released indicates an enthalpy change of 2251 kJ mol?1 (260 kcal mol?1). For this process, calculate the entropy change for the system and the entropy change for the surroundings.arrow_forward
- Chemosynthetic bacteria reduce CO2 by “splitting” H2S(g) instead of the H2O(g) used by photosynthetic organisms. Compare the free energy change for splitting H2S with that for splitting H2O. Is there an advantage to using H2S instead of H2O?arrow_forwardcells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as ATP(aq) + H2O(l)--> ADP(aq) + H2PO4-(aq). where ADP represent adenosine diphosphate. For this reaction, ΔG∘=-30.5kj/mol. a. If all the free energy from the metabolism of glucose goes into forming ATP from ADP, how many ATP molecules can be produced for every molecule of glucose? C6H12O6 + 6O2 → 6CO2 + 6H2Oarrow_forwardTRUE OR FALSE? 1. Entropy changes cannot be measured with a calorimeter like enthalpy changes. 2. If the result upon calculation of entropy changes in the universe is a positive value, the process is reactant-favored. 3. If the change in free energy, ΔG is negative, the reaction is spontaneous in the forward direction.arrow_forward
- Glycolysis is the process by which glucose is metabolized to lactic acid according to the equation C6H12O6(aq)2C3H6O3(aq) G=198 kJ at pH 7.0 and 25°C Glycolysis is the source of energy in human red blood cells. In these cells, the concentration of glucose is 5.0103 M, while that of lactic acid is 2.9103 M. Calculate AG for glycolysis in human blood cells under these conditions. Use the equation G=G+RT In Q, where Q is the concentration quotient, analogous to K.arrow_forwardFind the pKw of H2O and D2O at 60°C and 90°C (values in image). Write the balanced chemical reactions that pertain to these K values (values in image).arrow_forwardCells use the hydrolysis of adenosine triphosphate (ATP) as a source of energy. The conversion of ATP to ADP has a standard free-energy change of -30.5 kJ>mol. If all the free energy from the metabolism of glucose, C6H12O61s2 + 6 O21g2 ¡ 6 CO21g2 + 6 H2O1l2 goes into the conversion of ADP to ATP, how many moles of ATP can be produced for each mole of glucose?arrow_forward
- 1. Describe how you would calculate ∆G0′ for the reaction: glucose+ 6 O2 = 6 CO2 + 6 H2O. If you were told that this reaction is highlyexergonic, what would be the arithmetic sign (negative or positive)of the ∆G0′ you would expect for this reaction?arrow_forwardCalculate the standard free energy, ΔGo, for the following equation at 25.0 oC and determine if the reaction is favorable or unfavorable. C2H6(g) + 7Cl2(g) ⟶ 2CCl4(g) + 6HCl(g) Group of answer choices 720.2 kJ/mole, unfavorable -656.2 kJ/mole, favorable 720.2 kJ/mole, favorable -720.2 kJ/mole, unfavorable 19.7 kJ/mole, favorable -656.2 kJ/mole, unfavorable 656.2 kJ/mole, favorable -19.7 kJ/mole, favorable -720.2 kJ/mole, favorable -19.7 kJ/mole, unfavorable 656.2 kJ/mole, unfavorable 19.7 kJ/mole, unfavorablearrow_forwardThe change of state from gaseous H2O to liquid H2O has a ΔH of -9.72 kcal/mol and a ΔS of -26.1 cal/(mol·K). What is the change in free energy of this reaction at 200K?arrow_forward
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