Chemistry · Unit 3 · Chemical equilibrium systems · Chemical equilibrium
AI-marked practice questions tied to QCAA mark schemes for this exact LO. Free to start.
Start free practiceFull questions, answers and worked solutions unlock when you start a free practice session.
Consider the following equilibrium: $$\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g) \quad \Delta H = +58 \text{ kJ mol}^{-1}$$ A sample of the gas mixture at equilibrium is initially at a temperature of 298 K. (a) Predict the direction of equilibrium shift when the temperature is increased to 350 K. [1] (b) Explain your prediction using Le Châtelier's principle. [1]
Consider the equilibrium: \( N_2O_4(g) \rightleftharpoons 2NO_2(g) \quad \Delta H = +58 \text{ kJ/mol} \) Which change would shift the equilibrium position to the right?
Consider the equilibrium: $$\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g) \quad \Delta H = +57 \text{ kJ mol}^{-1}$$ Which change will shift the equilibrium position to the right?