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.
Explanation
(a) When the rate of forward reaction is equal to the rate of backward reaction. (b)(i) Increasing the temperature (ii) Decreasing the pressure (c) Le Chatelier's principle
