Problem: Consider the following equation for an electrochemical cell reaction.H2(s) + PbCI2(s) ⇌ Pb(s) + 2HCl(aq) Predict the immediate effect of the following changes on the observed cell voltage, E.Increased E          Decreased E          No change in Eincrease the temperaturedissolve NaOH into the solutionincrease the amount of PbCl2dilute the solution by adding H2O

FREE Expert Solution

The Gibbs free energy change determines the voltage of an electrochemical cell. This, in turn, depends on factors such as concentration, gas pressure, and temperature.

Equation 1:

G°=-RT ln K

ΔG° = Gibbs Free Energy, J
R = gas constant = 8.314 J/(molK)
T = temperature, K
K = equilibrium constant


Equation 2:

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Problem Details

Consider the following equation for an electrochemical cell reaction.

H2(s) + PbCI2(s) ⇌ Pb(s) + 2HCl(aq) 

Predict the immediate effect of the following changes on the observed cell voltage, E.

Increased E          Decreased E          No change in E

increase the temperature

dissolve NaOH into the solution

increase the amount of PbCl2

dilute the solution by adding H2O

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