Dinitrogen tetroxide decomposes to nitrogen dioxide according to the balanced…

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 decomposes to nitrogen dioxide according to the balanced equation

\mathrm{N_2O_4(g)} \rightleftharpoons 2\,\mathrm{NO_2(g)}

2.00\,\text{L}

rigid flask is charged at

350\,\text{K}

with

1.00\,\text{mol}

\mathrm{N_2O_4(g)}

and no

\mathrm{NO_2(g)}

. The equilibrium constant for the reaction at this temperature is

K_c = 0.012

. (a) Determine the molar concentration of each species immediately after the flask is sealed but before any reaction occurs. (b) Write algebraic expressions for the equilibrium concentrations of

\mathrm{N_2O_4(g)}

and

\mathrm{NO_2(g)}

in terms of a single variable that represents the extent of reaction. (c) Derive an equation involving that single variable and the given equilibrium constant, then solve for the variable algebraically (do not round intermediate values). (d) Using your solved value, calculate the equilibrium molar concentration of each gas. Verify that the calculated concentrations satisfy the equilibrium expression to an appropriate number of significant figures.

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