Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(a...

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Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(aq) -80 Consider the reaction: N2(g) + O2(g)—>2NO(g) Using standard thermodynamic data at 298K, calculate the free energy change when

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Answer 1

Answer #1

Given:

Gof(N2(g)) = 0.0 KJ/mol

Gof(O2(g)) = 0.0 KJ/mol

Gof(NO(g)) = 86.6 KJ/mol

Balanced chemical equation is:

N2(g) + O2(g) ---> 2 NO(g)

ΔGo rxn = 2*Gof(NO(g)) - 1*Gof( N2(g)) - 1*Gof(O2(g))

ΔGo rxn = 2*(86.6) - 1*(0.0) - 1*(0.0)

ΔGo rxn = 173.2 KJ

This is when 1 mol of N2 reacts.

So, for 1.60 mol,

ΔGo rxn = 173.2*1.60 KJ = 277.12 KJ

Answer: 277.12 KJ

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Answer 2

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Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(a...