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Equilibrium constant $K_p$ for homogeneous systems (A-level only)

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Question 2

The equation for the reversible decomposition of gaseous dinitrogen tetroxide to nitrogen dioxide is shown below:

N2O4(g)⇌2NO2(g)ΔH=+57 kJ mol−1 \text{N}_2\text{O}_4(\text{g}) \rightleftharpoons 2\text{NO}_2(\text{g}) \quad \Delta H = +57\text{ kJ mol}^{-1} N2​O4​(g)⇌2NO2​(g)ΔH=+57 kJ mol−1

Which statement about this system at equilibrium is correct?

The addition of a suitable catalyst increases the rate of the forward reaction relative to the reverse reaction, increasing the equilibrium yield of NO2\text{NO}_2NO2​.

A decrease in temperature, at constant pressure, decreases the value of the equilibrium constant KpK_pKp​.

An increase in total pressure, at constant temperature, increases the equilibrium yield of NO2\text{NO}_2NO2​.

The value of the equilibrium constant KpK_pKp​ increases when the total pressure of the system is increased at constant temperature.

Equilibrium constant $K_p$ for homogeneous systems (A-level only) Questions

  1. A Level
  2. /Chemistry
  3. /Equilibrium constant $K_p$ for homogeneous systems (A-level only)