Question

Calculate ΔGrxn at 35 ∘C. for the following reactions: 2CH4(g)→C2H6(g)+H2(g) 2NH3(g)→N2H4(g)+H2(g) N2(g)+O2(g)→2NO(g) 2KClO3(s)→2KCl(s)+3O2(g)

Calculate ΔGrxn at 35 ∘C. for the following reactions: 2CH4(g)→C2H6(g)+H2(g) 2NH3(g)→N2H4(g)+H2(g) N2(g)+O2(g)→2NO(g) 2KClO3(s)→2KCl(s)+3O2(g)

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Answer #1

ΔGrxn = ΔGform products - ΔGform reactants

= -32.1 - (2 * 68.4) KJ/mol

= -168.9 KJ/mol

part b

ΔGrxn= ΔGform products - ΔGform reactants

ΔGrxn= 120.3 - (-2* 16.4) = 153.1 KJ/mol

ΔGform H2= 0 because H2 is standard state of Hydrogen.

part c

ΔGrxn = 2 * ΔGformNO

because nitrogen and oxygen are in their standard states

= 2*86.6 KJ/mol = 137.2 KJ/mol

part d

ΔGrxn = [2ΔGf(KCl (s)) + 3ΔGf(O2 (g))] - [2ΔGf(KClO3 (s))]

[2(-408.32) + 3(0)] - [2(-289.91)] = -236.82 kJ

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