Reversible Reactions (GCSE Chemistry)

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

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?

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

When gases A and B react to equilibrium A ? B and the equilibrium is exothermic forward, adding heat is equivalent to:

For the exothermic equilibrium P ? Q + heat, what action would increase the amount of Q at equilibrium?

How does adding more product to an equilibrium mixture immediately affect the reaction rates?

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

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

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?

Which change will increase the rate of both the forward and reverse reactions but will NOT change the position of a chemical equilibrium?

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