Chapter 3, Problem 17P

Interpretation Introduction

(a) Interpretation:

If the $\Delta S^o$for the given reaction is less than or greater than zero should be identified.

Concept Introduction:

The entropy of the reaction defines the randomness of the system. The value of change in entropy will be positive if randomness in the system (reaction) increases and it has negative value if randomness decreases.

Interpretation Introduction

(b) Interpretation:

The non-equilibrium concentration of ethanol in yeast cells, if the value of change in Gibbs free energy is $-38.3\text{ kJ/mol}$at pH 7.4 and temperature $37{}^o\text{C}$

Concept Introduction:

The standard Gibbs free energy is related to standard electrode potential of cell as follows:

$\Delta G^o=-nF{E}^o\left(\text{V}\right)$Here, n is number of electrons transferred in the overall reaction and F is Faradays constant which is $96500{\text{ C mol}}^{\text{-1}}$.

Also, standard change in Gibbs free energy is related to change in Gibbs free energy as follows:

$\Delta G=\Delta G^o+RT\ln \frac{\left[\text{P}\right]}{\left[\text{R}\right]}$Here, R is Universal gas constant; T is temperature, $\left[\text{P}\right]$ is concentration of product and $\left[\text{R}\right]$ is concentration of reactant.

Interpretation Introduction

(c) Interpretation:

The effect on value of change in Gibbs free energy due to decrease in pH should be identified.

Concept Introduction:

Standard change in Gibbs free energy is related to change in Gibbs free energy as follows:

$\Delta G=\Delta G^o+RT\ln \frac{\left[\text{P}\right]}{\left[\text{R}\right]}$Here, R is Universal gas constant; T is temperature, $\left[\text{P}\right]$ is concentration of product and $\left[\text{R}\right]$ is concentration of reactant.

Interpretation Introduction

(d) Interpretation:

The effect on value of change in Gibbs free energy due to increase in intracellular CO₂levels should be identified.

Concept Introduction:

Standard change in Gibbs free energy is related to change in Gibbs free energy as follows:

$\Delta G=\Delta G^o+RT\ln \frac{\left[\text{P}\right]}{\left[\text{R}\right]}$Here, R is Universal gas constant; T is temperature, $\left[\text{P}\right]$ is concentration of product and $\left[\text{R}\right]$ is concentration of reactant.

Interpretation Introduction

(e) Interpretation:

The effect on value of change in standard Gibbs free energy due to increase in intracellular CO₂levels should be identified.

Concept Introduction:

Standard change in Gibbs free energy is related to change in Gibbs free energy as follows:

$\Delta G=\Delta G^o+RT\ln \frac{\left[\text{P}\right]}{\left[\text{R}\right]}$Here, R is Universal gas constant; T is temperature, $\left[\text{P}\right]$ is concentration of product and $\left[\text{R}\right]$ is concentration of reactant.