What is $\Delta$_rG° at 500.0 K for the following reaction? Zn(s)+ H₂O(g)$\to$ ZnO(s)+ H₂(g) A) 80.7 kJ/mol-rxn B) -80.7 kJ/mol-rxn C) 92.0 kJ/mol-rxn D) -92.0 kJ/mol-rxn E) -136.7 kJ/mol-rxn

Question

Quizplus · Accepted Answer

The Gibbs free energy change (ΔG°) can be calculated using the equation ΔG° = ΔH° - TΔS°. First, calculate ΔH° and ΔS° for the reaction using the given standard enthalpies and entropies of formation. Then, apply the equation at 500.0 K to find ΔG°.

What Is Δ\DeltaΔ rG° at 500 →\to→ ZnO(s)+ H2(g) A) 80

What Is $\Delta$ _rG° at 500 $\to$ ZnO(s)+ H₂(g)

A) 80