Reversible Reactions (GCSE Chemistry)

Which change will increase the percentage yield of product at equilibrium for a given reversible reaction?

A student carries out a reversible gas reaction in a closed container and increases the container temperature. Immediately the concentration of product increases but later drops to a lower value than before the temperature change. Is this possible?

In the Haber process (N2 + 3H2 ? 2NH3, exothermic), the industrial compromise uses high pressure, moderate temperature and an iron catalyst. Why is a moderate (not lowest possible) temperature used?

If the forward reaction is endothermic, what effect does increasing temperature have on the equilibrium constant K?

Which of the following is an accurate short Le Chatelier statement?

For the exothermic reversible reaction A + B ? C + heat, Le Chatelier’s principle predicts that increasing the temperature will:

A reversible reaction reached equilibrium in a sealed vessel. Which of these would definitely change the equilibrium constant K at that temperature?

Which description best differentiates reaction rate and equilibrium yield?

Which experimental change would increase the rate but reduce the maximum yield for an exothermic forward reaction?

Which statement about catalysts is correct?

A certain reversible reaction is endothermic in the forward direction. When the system is cooled, the equilibrium will: