Chapter 18, Problem 133CP

(a)

Interpretation Introduction

Interpretation: The work done to transport 1.0 mole of ${\text{K}}^{\text{+}}$ from the blood to the inside of a muscle cell at 37°C needs to be determined. The concentration of ${\text{K}}^{\text{+}}$ in the muscles cells is 0.15 M and the concentration of ${\text{K}}^{\text{+}}$ in blood plasma is 0.0050 M.

Concept Introduction:

Thermodynamic is mainly deals with the enthalpy, entropy and Gibb’s energy of the system. The enthalpy of system indicates the energy or heat content of a system whereas entropy of system indicates the randomness of constitute particles in the system.

For a spontaneous reaction, the $\Delta \text{G }$ has a negative value with large value of equilibrium constant K. On the contrary, for a non-spontaneous reaction, the $\Delta \text{G }$ has a positive value with small value of equilibrium constant K.

(b)

Interpretation Introduction

Interpretation: The probability of transportation of ${\text{K}}^{\text{+}}$ needs to be determined when 1.0 moles of ${\text{K}}^{\text{+}}$ is transferred from blood to the cell.

Concept Introduction:

Thermodynamic is mainly deals with the enthalpy, entropy and Gibb’s energy of the system. The enthalpy of system indicates the energy or heat content of a system whereas entropy of system indicates the randomness of constitute particles in the system.

For a spontaneous reaction, the $\Delta \text{G }$ has a negative value with large value of equilibrium constant K. On the contrary, for a non-spontaneous reaction, the $\Delta \text{G }$ has a positive value with small value of equilibriumconstant K.

(c)

Interpretation Introduction

Interpretation: The moles of ATP that must be hydrolyzed to provide the energy for the transport of 1.0 moles of ${\text{K}}^{\text{+}}$ under standard condition for the ATP hydrolysis reaction needs to be determined.

  ${\text{ATP}}_{\text{(aq)}}{\text{+ H}}_{\text{2}}{\text{O}}_{\text{(l)}}\stackrel{}{\to }{\text{ ADP}}_{\text{(aq)}}{\text{ + H}}_{\text{2}}{\text{PO}}_{\text{4}}{{}^{\text{-}}}_{\text{(aq)}}\text{ K = 1}{\text{.7×10}}^{\text{5}}\text{ (at37°C)}$

Concept Introduction:

Thermodynamic is mainly deals with the enthalpy, entropy and Gibb’s energy of the system. The enthalpy of system indicates the energy or heat content of a system whereas entropy of system indicates the randomness of constitute particles in the system.

For a spontaneous reaction, the $\Delta \text{G }$ has a negative value with large value of equilibrium constant K. On the contrary, for a non-spontaneous reaction, the $\Delta \text{G }$ has a positive value with small value of equilibriumconstant K.