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441E2||Q4|5

The Gibbs energy of formation of any chemical element in its reference state is

= 0

None of these

� 0

Absolute value of the Galvani potential difference (electrical potential difference between two phases)

Can be thermodynamically calculated

Is unknown

Is known

When temperature increases, the standard OCP of a H /O fuel cell

Decreases

Does not change

Increases

If one uses data of Chapter 10: Data Section, it can be found that when temperature increases, the standard Gibbs energy a C(s)/O (g) fuel cell reaction

Increases

Decreases

Does not change

If a fuel cell reaction is (1/2) CH4 (g) + O2 (g) = (1/2) CO2 (g) + H2O(g), the standard Gibbs energy of the reaction is defined as

ΔfG (H2O,g) + 0.5 Δ G (CO2 ,g) + 0.5 Δ G (CH4 ,g) + Δ G (O2 ,g)

ΔfG (H2O,g) + Δ G (CO2 ,g) - Δ G (CH4 ,g) - Δ G (O2 ,g)

ΔfG (H2O,g) + 0.5 Δ G (CO2 ,g) - 0.5 Δ G (CH4 ,g) - Δ G (O2 ,g)

The precise relationship between Gibbs energy (Δ G), enthalpy (Δ H), and entropy (Δ S) of a chemical reaction at temperature T is

ΔrG(T) = ΔrH(T) + T ΔrS(T)

Δ G(T) = Δ H(T) – T Δ S(T)

ΔrG(T) = ΔrH(To) – T ΔrS(To), where To = 298.15 K

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