At 700 K the decomposition of dinitrogen tetroxide occurs 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

At 700 K the decomposition of dinitrogen tetroxide occurs according to the balanced equation

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

A rigid 1.50 L container is charged with 0.240 mol

\mathrm{N_2O_4}

and 0.800 mol

\mathrm{NO_2}

. After the system reaches equilibrium the mixture is found to contain 0.650 mol

\mathrm{NO_2}

. Assume the temperature remains constant and no other gases are present. (1) Calculate the initial molar concentration of each species in the container. (2) Determine the change in the amount (in moles) of

\mathrm{NO_2}

that occurs as the system moves from the initial state to equilibrium. Clearly indicate the algebraic sign of this change. (3) Determine the equilibrium molar concentrations of

\mathrm{N_2O_4}

and

\mathrm{NO_2}

. (4) Using the equilibrium concentrations you obtained, calculate the numerical value of the equilibrium constant

K_c

at 700 K. Include the correct unit or state that it is dimensionless, and report your answer with an appropriate number of significant figures.

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