For the reaction below, determine the standard free energy change, δg o. cu(s) + sn2+(aq) → cu2+(aq) + sn(s) e o cell =–0.48 v view available hint(s) for the reaction below, determine the standard free energy change, δg o. cu(s) + sn2+(aq) → cu2+(aq) + sn(s) e o cell =–0.48 v −92.6 kj 92.6 kj −46.3 kj 46.3 kj

92.6 kJ.

Explanation:

∵ ΔG°rxn = - nFE°cell,

Where, ΔG°rxn is the standard free energy change (J).

n is the no. of electrons in the reaction (n =2).

F is Faraday constant (C/mol) (F = 96500 C/mol).

E°cell is the standard cell potential (E°cell = - 0.48 V).

∴ ΔG°rxn = - nFE°cell = - (2)(96500 C/mol)(- 0.48 V) = 92640 J = 92.64 kJ.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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