Consider the reaction represented by the following Q equation: N\(_2\)O\(_{4(g)}\) \(\rightleftharpoons\) 2NO\(_{2(g)}\) \(\Delta\)H = +57.2KJmol\(^{-1}\) (...
Question 1 Report
Consider the reaction represented by the following Q equation: N\(_2\)O\(_{4(g)}\) \(\rightleftharpoons\) 2NO\(_{2(g)}\) \(\Delta\)H = +57.2KJmol\(^{-1}\)
(a) When is the reaction said to be at equilibrium?
(b) Mention two conditions that can favour the forward reaction
(c) Name the principle involved in (b) above.
Answer Details
(a) The reaction is at equilibrium when the rate of the forward reaction equals the rate of the reverse reaction, so that the concentrations of N2O4 and NO2 remain constant (a dynamic equilibrium).
(b) The forward reaction is endothermic (ΔH = +57.2 kJ mol-1) and produces more moles of gas (1 → 2). Two conditions that favour it are:
- Increasing the temperature.
- Decreasing the pressure (increasing the volume).
(Removing NO2 as it forms would also favour it.)
(c) The principle involved is Le Chatelier's principle.
Download The App On Google Playstore
Everything you need to excel in your exams
