We're being asked to calculate the change in Gibbs free energy for each of the following sets of ΔH°_{rxn}, ΔS°_{rxn}, and T.

We can calculate the change in **Gibbs free energy (**** ΔG°_{rxn}) **using the following equation:

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\u2206}}{\mathbf{H}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{-}}{\mathbf{T}}{\mathbf{\u2206}}{\mathbf{S}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}}$

Note that we need to convert J/K into kJ/K since we need ΔG˚ in kJ/mol.

**Part 1. ΔH° _{rxn}= 88 kJ , ΔS°_{rxn}= 154 J/K , T= 292 K**

Calculate the change in Gibbs free energy for each of the following sets of ΔH°_{rxn}, ΔS°_{rxn}, and T.

Part 1

ΔH°_{rxn}= 88 kJ , ΔS°_{rxn}= 154 J/K , T= 292 K

Express your answer using two significant figures.

Part 2

ΔH°_{rxn}= 88 kJ , ΔS°_{rxn}= 154 J/K , T= 755 K

Express your answer using two significant figures.

Part 3

ΔH°_{rxn}= 88 kJ , ΔS°_{rxn}=− 154 J/K , T= 292 K

Express your answer using two significant figures.

Part 4

ΔH°_{rxn}=− 88 kJ , ΔS°_{rxn}= 154 J/K , T= 408 K

Express your answer using two significant figures.

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