Consider the following two equilibria at a given temperature

CHEMISTRY · Single correct · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

Consider the following two equilibria at a given temperature. 1. N2O4(g)  ⇌  2 NO2(g)\mathrm{N_2O_4}(g)\;\rightleftharpoons\;2\,\mathrm{NO_2}(g) K1=4.6×10−3K_1 = 4.6\times10^{-3} 2. 2 NO2(g)  ⇌  2 NO(g)+O2(g)2\,\mathrm{NO_2}(g)\;\rightleftharpoons\;2\,\mathrm{NO}(g)+\mathrm{O_2}(g) K2=1.2×102K_2 = 1.2\times10^{2} What is the equilibrium constant for the overall reaction N2O4(g)  ⇌  2 NO(g)+O2(g)\mathrm{N_2O_4}(g)\;\rightleftharpoons\;2\,\mathrm{NO}(g)+\mathrm{O_2}(g) under the same conditions? (a) 2.6×1012.6\times10^{1} (b) 5.5×10−55.5\times10^{-5} (c) 5.5×10−15.5\times10^{-1} (d) 2.6×10−22.6\times10^{-2}

Related theory

Browse the problem library