For the gaseous reaction: N 2 O 4 ⇌ 2NO 2 , the following thermodynamical data are given Δ H ° 300 K = +57.0 kJ mol -1 ; Δ S ° 300 K = +0.176 kJ K -1 mol -1 Δ H ° 600 K = +58.0 kJ mol -1 ; Δ S ° 600 K

Question

For the gaseous reaction: N 2 O 4 ⇌ 2NO 2 , the following thermodynamical data are given Δ H ° 300 K = +57.0 kJ mol -1 ; Δ S ° 300 K = +0.176 kJ K -1 mol -1 Δ H ° 600 K = +58.0 kJ mol -1 ; Δ S ° 600 K = +0.178 kJ K -1 mol -1 Assuming partial pressure of each component is 1 bar, the direction of spontaneous reaction is/are

TestHub · Accepted Answer

With every partial pressure 1 bar, Q = 1 and the direction is given by the sign of Δ G^° Δ G^°₃₀₀ = 57.0 - (300)(0.176) = 57.0 - 52.8 = +4.2 kJ/mol, positive, so the reaction is backward

Δ G^°₆₀₀ = 58.0 - (600)(0.178) = 58.0 - 106.8 = -48.8 kJ/mol, negative, so the reaction is forward

The correct options are (b) and (c).

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