Nitrogen monoxide reacts reversibly with oxygen.
2NO(g)+O2(g)⇌2NO2(g) 2\text{NO(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)} 2NO(g)+O2(g)⇌2NO2(g)For the quantities shown in the equation, the reaction from left to right gives out 114 kJ of energy.
What can be deduced about the energy transfer when the reaction goes from right to left?
It is exothermic and 114 kJ114\ \text{kJ}114 kJ of energy is given out
It is exothermic and more than 114 kJ114\ \text{kJ}114 kJ of energy is given out
It is endothermic and less than 114 kJ114\ \text{kJ}114 kJ of energy is taken in
It is endothermic and 114 kJ114\ \text{kJ}114 kJ of energy is taken in
109 exam-style questions on AQA GCSE Chemistry 6.2 Reversible reactions and dynamic equilibrium, covering 6.2.1 Reversible reactions, 6.2.2 Energy changes and reversible reactions, 6.2.3 Equilibrium, 6.2.4 The effect of changing conditions on equilibrium, 6.2.5 The effect of changing concentration, 6.2.6 The effect of temperature changes on equilibrium, and 6.2.7 The effect of pressure changes on equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.