M3 Equilibrium Q&A
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Describe and explain, using le Chatelier’s principle, the effect of an increase in temperature on the position of equilibrium on the following reaction:
• Forward reaction is exothermic • (When temperature is increased) the position of equilibrium shifts to the left • To minimise the effects of the increase in temperature by absorbing energy
Describe and explain, using le Chatelier’s principle, the effect of an increase in pressure on the position of equilibrium on the following reaction:
• There are more gaseous moles of reactants than products (more gaseous moles on the left hand side) • (When pressure is increased) the position of equilibrium shifts to the right • To minimise the effects of the increase in pressure by reducing the pressure
Describe and explain, using le Chatelier’s principle, the effect of the addition of a catalyst on the position of equilibrium:
• Catalyst increases the rate of the forward and reverse reactions equally • No effect on the position of equilibrium
What is the advantage of a high percentage yield?
• Shows that there is little waste in the starting materials • Efficient conversion of reactants to products
What is the advantage of a high atom economy?
• Shows that there is little waste products • More of the desired product • 100% atom economy when there is only one product (addition reaction) • Lower atom economy when there is a by-product (substitution reaction) • Atom economy can be increased by finding a use for the by-product