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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

Carbon monoxide is toxic because it bonds much more strongly to the iron in hemoglobin (Hgb) than does O2. Consider the following reactions and approximate standard free energy changes:

Hgb + O 2 HgbO 2 Δ G = 70 KJ Hgb + CO HgbCO Δ G = 80 KJ

Using these data, estimate the equilibrium constant value at 25°C for the following reaction:

HgbO 2 + CO HgbCO + O 2

Interpretation Introduction

Interpretation: The formation reaction of HgbO2,HgbCO and their ΔG° value is given. The value of K is to be calculated at given temperature for the reaction between HgbO2 and CO .

Concept introduction: Equilibrium constant K , is defined as the ratio of the concentration of products to that of the reactants at equilibrium. If a given reaction is at equilibrium, the free energy change is,

ΔG=0Q=K

The expression for standard free energy change is,

ΔG°=RTln(K)

Explanation

Explanation

Given

The stated reaction is,

HgbO2+COHgbCO+O2

For the reaction,

Hgb+O2HgbO2

The value of ΔG° is 70kJ .

The reverse reaction of the above equation is,

HgbO2Hgb+O2 (1)

The value of ΔG° is 70kJ .

For the reaction,

Hgb+COHgbCO (2)

The value of ΔG° is 80kJ .

Addition of equation (1) and (2) will give the required stated reaction. The resultant value of ΔG° from equation (1) and (2) is,

(80+70)kJ=10kJ_

The value ΔG° for the given reaction is 10kJ .

Given temperature is 25°C .

The conversion of kilo-joule (kJ) into joule (J) is done as,

1kJ=103J

Hence,

The conversion of 10kJ into joule is,

10kJ=(10×103)J=10×103<

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