# The rote of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μ mol/L. (A hemoglobin concentration of 2.21 μ mol/L is equal to 2.21 × 10 −6 mol/L.) [Hb] 0 ( μ mol/L) [CO] 0 ( μ mol/L) Initial Rate ( μ mol/L · s) 2.21 1.00 0.619 4.42 1.00 1.24 4.42 3.00 3.71 a. Determine the orders of this reaction with respect to Hb and CO. b. Determine the rate law. c. Calculate the value of the rate constant. d. What would be the initial rate for an experiment with [Hb] 0 = 3.36 μ mol/L and [CO] 0 = 2.40 μ mol/L?

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

Chapter
Section

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 11, Problem 35E
Textbook Problem
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## The rote of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 × 10−6 mol/L.) [Hb]0(μmol/L) [CO]0(μmol/L) Initial Rate (μmol/L · s) 2.21 1.00 0.619 4.42 1.00 1.24 4.42 3.00 3.71 a. Determine the orders of this reaction with respect to Hb and CO.b. Determine the rate law.c. Calculate the value of the rate constant.d. What would be the initial rate for an experiment with [Hb]0 = 3.36 μmol/L and [CO]0 = 2.40 μmol/L?

(a)

Interpretation Introduction

Interpretation: The data related to the rate of reaction at different initial concentrations of [Hb] and [CO] is given for the reaction between hemoglobin (Hb) and carbon monoxide (CO) . The orders of the reaction with respect to Hb and CO , rate law, the value of the rate constant and the initial rate of the reaction for the given values of concentration of [Hb] and [CO] are to be calculated.

Concept introduction: The relation between the reaction rate and the concentration of the reactants is stated by the rate law.

### Explanation of Solution

The rate law for the given reaction is calculated by the expression,

Rate=k[Hb]m[CO]n

Where,

• [Hb] and [CO] are the concentrations of Hb and CO .
• k is the rate constant.

The values of m and n are calculated by the comparison of the different rate values from the given table.

The value of m is calculated using the first and second result. Substitute the values of the concentration of [Hb] and [CO] for the first two experiments in the above expression.

Rate1=k[2.21]m[1.00]n

Rate2=k[4.42]m[1.00]n

According to the given rate values in the table,

Rate2Rate1=1.24μmol/Ls0.619μmol/Ls

Therefore,

k[4.42]m[1.00]nk[2.21]m[1.00]n=1.24μmol/Ls0.619μmol/Ls(2)m=2m=1_

The value of n is calculated using the second and third result

(b)

Interpretation Introduction

Interpretation: The data related to the rate of reaction at different initial concentrations of [Hb] and [CO] is given for the reaction between hemoglobin (Hb) and carbon monoxide (CO) . The orders of the reaction with respect to Hb and CO , rate law, the value of the rate constant and the initial rate of the reaction for the given values of concentration of [Hb] and [CO] are to be calculated.

Concept introduction: The relation between the reaction rate and the concentration of the reactants is stated by the rate law.

(c)

Interpretation Introduction

Interpretation: The data related to the rate of reaction at different initial concentrations of [Hb] and [CO] is given for the reaction between hemoglobin (Hb) and carbon monoxide (CO) . The orders of the reaction with respect to Hb and CO , rate law, the value of the rate constant and the initial rate of the reaction for the given values of concentration of [Hb] and [CO] are to be calculated.

Concept introduction: The relation between the reaction rate and the concentration of the reactants is stated by the rate law.

To determine: The value of the rate constant, k .

(d)

Interpretation Introduction

Interpretation: The data related to the rate of reaction at different initial concentrations of [Hb] and [CO] is given for the reaction between hemoglobin (Hb) and carbon monoxide (CO) . The orders of the reaction with respect to Hb and CO , rate law, the value of the rate constant and the initial rate of the reaction for the given values of concentration of [Hb] and [CO] are to be calculated.

Concept introduction: The relation between the reaction rate and the concentration of the reactants is stated by the rate law.

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