The reversible reaction is at equilibrium in a flask at

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

Problem

The reversible reaction

\mathrm{N_2O_4(g)\;\rightleftharpoons\;2NO_2(g)}\qquad (\Delta H=+57\,kJ\,mol^{-1})

is at equilibrium in a

2.0\,\mathrm{L}

flask at

298\,\mathrm{K}

. Five separate stresses are then applied, one at a time. A. Warm the flask to

308\,\mathrm{K}

. B. Decrease the flask volume to

1.0\,\mathrm{L}

. C. Rapidly remove

\tfrac{1}{4}

of the

\mathrm{NO_2(g)}

present. D. Add sufficient inert argon to raise the total pressure by

0.50\,\mathrm{atm}

at constant volume. E. Dilute the gas mixture by attaching an evacuated

2.0\,\mathrm{L}

bulb (isothermal). (i) Rank the stresses from greatest to least predicted increase in the equilibrium partial pressure of

\mathrm{NO_2(g)}

. (ii) In 2–3 sentences, justify why the stress you ranked first produces a larger increase than the stress you ranked second.

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