Under standard conditions at 25 °C, the reaction ½ N 2 (g) + ½ O 2 (g) à NO(g) h

Question

Under standard conditions at 25 °C, the reaction ½ N2(g) + ½ O2(g) à NO(g) has G° = +27.5 kJ/mol.

For the non-standard initial conditions, P(N2) = 1.0 bar, P(O2) = 1.0 bar, P(NO) = 10.0 bar at the same temperature, this reaction is:

Under standard conditions at 25 C, the reaction N2 (g) O2 (g) NO(g) has AG +27.5 kJ/mol. For the non-standard initial conditions, P(N2) 1.0 bar, P(O2) 1.0 bar, P(NO) -10.0 bar at the same temperature, this reaction is Spontaneous in the forward direction, because K 1 Spontaneous in the forward direction, because AG is a negative value Spontaneous in the reverse direction, because AG is a positive value Spontaneous in the reverse direction, because K 1

Explanation / Answer

For the given reaction,

dGo represents spontaneity of a chemical reaction.

When dGo is ve, the reaction is spontaneous in the forward direction, whereas, when the value of dGo is -ve, the reaction is negative in the forward direction.

Thus, here with a +ve dGo value, the reaction would be,

-Spontaneous in the reverse direction, because dG is a positive value

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