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

**Equation 1:**

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{\xb0}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RT}}{\mathbf{}}{\mathbf{ln}}{\mathbf{}}{\mathbf{K}}}$

ΔG° = Gibbs Free Energy, J

R = gas constant = 8.314 J/(mol∙K)

T = temperature, K

K = equilibrium constant

**Equation 2:**

Consider the following equation for an electrochemical cell reaction.

H_{2}(s) + PbCI_{2}(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 PbCl_{2}

dilute the solution by adding H_{2}O

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