The Effect Of Changing Conditions On Equilibrium (ht Only) (GCSE Chemistry)

In a gaseous equilibrium with more moles of gas on the left, increasing pressure will:

Which experimental action would change the rate but not the equilibrium position for a closed heterogeneous system?

Which description correctly distinguishes rate and extent of reaction?

For the reversible reaction A(g) ? 2B(g), what is the effect of removing some B continuously?

Which change will increase the extent of a reaction that is endothermic in the forward direction?

If an equilibrium is endothermic in the forward direction, what will happen to K when temperature is raised?

For the gas equilibrium CO(g) + 2H2(g) ? CH3OH(g), what is the effect of increasing total pressure (by decreasing volume) on the position of equilibrium?

Which experimental change would increase the rate but not change the equilibrium position for a given reversible reaction?

A student heats an exothermic reversible reaction until equilibrium is reached, then increases the temperature further. What happens to the yield of products?

For the equilibrium H2(g) + I2(g) ? 2HI(g), which change will decrease the equilibrium concentration of HI?

Which effect does doubling the concentration of a reactant have immediately on the rates at equilibrium?