Reversible Reactions (GCSE Chemistry)

A reversible gas reaction has fewer moles of gas on the product side than on the reactant side. Increasing the pressure (by decreasing the container volume) will:

In a reversible reaction, why might chemists accept a lower equilibrium yield in industry rather than using conditions that give the highest possible yield?

Which statement correctly compares rate of reaction and extent (yield)?

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

For the equilibrium N2 + 3H2 ? 2NH3 (exothermic forward), which change would increase the equilibrium yield of ammonia (NH3)?

In an equilibrium involving gases, which factor would NOT affect the position of equilibrium?

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

Which of the following describes why increasing pressure can change the extent of a gas-phase equilibrium?

Which of these describes why changing concentration shifts an equilibrium?

Which of the following changes will increase the equilibrium yield of products for an endothermic forward 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?