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.

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation: