The Effect Of Temperature Changes On Equilibrium (ht Only) (GCSE Chemistry)

For the reversible reaction A(g) ? B(g), ?H° forward = -120 kJ. If the temperature is reduced, the equilibrium constant K will:

A system at equilibrium is exothermic in the forward direction. Which change would increase the equilibrium yield of products?

Which practical change in an industrial exothermic equilibrium reactor would increase product yield without changing temperature?

For the equilibrium A ? B, a decrease in temperature causes the position to move to the left. The forward reaction is therefore:

For the gas equilibrium 2NO2(g) ? N2O4(g), the forward reaction is exothermic. If the temperature is increased and pressure held constant, the equilibrium colour changes from brown to:

A system at equilibrium is exothermic forward. Which of these will increase the product yield most dramatically?

Consider the reaction N2(g) + 3H2(g) ? 2NH3(g), which is exothermic forward. Increasing temperature in the Haber process will:

A student measures equilibrium concentrations at two temperatures and finds K1 > K2 where K1 is at lower temperature. The forward reaction must be:

If an equilibrium constant Kc for the reaction A + B ? C + D decreases when temperature is increased, the forward reaction is:

Which of the following is a correct industrial strategy when an equilibrium reaction is exothermic and the desired product has fewer gas moles than the reactants?

When a reaction is exothermic in the forward direction, which of these changes will increase K (equilibrium constant) for the forward reaction?