Dinitrogen tetroxide and nitrogen dioxide interconvert according to N_2O_4(g)…

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

Problem

Dinitrogen tetroxide and nitrogen dioxide interconvert according to N2O4(g)⇌2NO2(g)\mathrm{N_2O_4(g) \rightleftharpoons 2NO_2(g)} At 298 K the equilibrium constant is Kc=4.6×10−3K_c = 4.6\times10^{-3}. A 2.00-L sealed flask at this temperature contains the following initial amounts: • nN2O4=0.0120 moln_{\mathrm{N_2O_4}}=0.0120\,\text{mol} • nNO2=0.00200 moln_{\mathrm{NO_2}} = 0.00200\,\text{mol} (a) Calculate the value of the reaction quotient QcQ_c for the initial mixture. Show all work, including concentration calculations. (b) Compare the value of QcQ_c you calculated in part (a) to the equilibrium constant KcK_c, and determine the direction in which the net reaction will proceed. Clearly state whether N2O4\mathrm{N_2O_4} is consumed or produced as the system moves toward equilibrium.

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