At 1000 K, the forward reaction has a negative value: 2 NO _2( g ) 2 NO ( g ) + O _2(…

CHEMISTRY · Single correct · A Level · Chemistry · Thermodynamics · Thermodynamics

Problem

At 1000 K, the forward reaction has a negative ΔG∘\Delta G^\circ value: 2NO2(g)⇌2NO(g)+O2(g)2\text{NO}_2(\text{g}) \rightleftharpoons 2\text{NO}(\text{g}) + \text{O}_2(\text{g}) Which expression is correct for the equilibrium at this temperature? (1) [NO2]2>[NO]2[O2][\text{NO}_2]^2 > [\text{NO}]^2[\text{O}_2] (2) [NO2]<[NO][\text{NO}_2] < [\text{NO}] (3) [NO]=2[O2][\text{NO}] = 2[\text{O}_2] (4) K>1K > 1

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