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# Problem: Consider the oxidation of NO to NO2 :NO(g) + 1/2O2(g) → NO2(g) Reactant or product  ΔH°f(kJ/mol)  S°(J/mol•K)  NO 91.3 210.8 O2 0 205.2 NO2 33.2 240.1Part ACalculate ΔG∘rxn at 25∘C. Express your answer with the appropriate units.Part BDetermine whether the reaction is spontaneous at standard conditions.

###### FREE Expert Solution

NO(g) + 1/2 O2(g) → NO2(g)

We’re given the ΔH˚f and S˚ of each reactant and product:

 Reactant or product ΔH°f(kJ/mol) S°(J/mol•K) NO 91.3 210.8 O2 0 205.2 NO2 33.2 240.1

Part 1:

We can use the following equation to solve for ΔG˚rxn:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{-}}{\mathbf{T\Delta S}}{{\mathbf{°}}}_{{\mathbf{rxn}}}}$

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###### Problem Details

Consider the oxidation of NO to NO2 :

NO(g) + 1/2O2(g) → NO2(g)

 Reactant or product ΔH°f(kJ/mol) S°(J/mol•K) NO 91.3 210.8 O2 0 205.2 NO2 33.2 240.1

Part A

Calculate ΔG∘rxn at 25∘C. Express your answer with the appropriate units.

Part B

Determine whether the reaction is spontaneous at standard conditions.

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