The endothermic reaction N_2O_4(g) 2 ,NO_2(g) has (K_c = 4.6 10^ -3 ) at 298 K and…

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

Problem

The endothermic reaction N2O4(g)⇌2 NO2(g)\mathrm{N_2O_4(g) \rightleftharpoons 2\,NO_2(g)} has Kc=4.6×10−3K_c = 4.6 \times 10^{-3} at 298 K and Kc=1.0×10−1K_c = 1.0 \times 10^{-1} at 350 K. A sealed container is at 298 K with an equilibrium mixture having [N2O4]=0.400 M[\mathrm{N_2O_4}] = 0.400\,\text{M} and [NO2]=0.043 M.[\mathrm{NO_2}] = 0.043\,\text{M}. The temperature is then rapidly raised to 350 K; the concentrations do not change during the temperature jump. What will be the concentration of NO2\mathrm{NO_2} after the system reaches the new equilibrium at 350 K? (a) 0.24 M0.24\,\text{M} (b) 0.18 M0.18\,\text{M} (c) 0.10 M0.10\,\text{M} (d) 0.20 M0.20\,\text{M}

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