The gas-phase reaction NO(g) + 12 ,O_2(g) NO_2(g) has an equilibrium constant at 298 ,K.

CHEMISTRY · Multi-part · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

The gas-phase reaction NO(g)+12 O2(g)→NO2(g)\mathrm{NO(g) + \tfrac12\,O_2(g) \rightarrow NO_2(g)} has an equilibrium constant K1=4.6×105K_1 = 4.6 \times 10^{5} at 298\,K. (a) Determine the numerical value of the equilibrium constant K2K_2 for the reaction 2 NO(g)+O2(g)→2 NO2(g)\mathrm{2\,NO(g) + O_2(g) \rightarrow 2\,NO_2(g)} written with all coefficients multiplied by 2. (b) Determine the equilibrium constant K3K_3 for the reaction NO2(g)→NO(g)+12 O2(g)\mathrm{NO_2(g) \rightarrow NO(g) + \tfrac12\,O_2(g)} obtained by reversing the original equation. (c) For both rewritten reactions, explain how the changes you made to the balanced equation lead to the numerical relationships among K1, K2,K_1,\,K_2, and K3K_3.

Related theory

Browse the problem library