2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants...

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2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants...

2Ca(s)+O2(g) → 2CaO(s)
ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K

For this problem, assume that all reactants and products are in their standard states.

Calculate the free energy change for the reaction at 17 ∘C.

Express your answer using four significant figures.

ΔG = _____kJ

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Answer 1

Answer #1

ΔHorxn = -1269.8 KJ/mol

ΔSorxn = -364.6 J/mol.K

= -0.3646 KJ/mol.K

T= 17.0 oC

= (17.0+273) K

= 290 K

use:

ΔGorxn = ΔHorxn - T*ΔSorxn

ΔGorxn = -1269.8 - 290 * (-0.3646)

ΔGorxn = -1164 KJ

Answer: -1164 KJ

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Answer 2

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