Rates of reactions

set answers

effect of Increasing temperature on rate

• particles gain KE

• Particles move faster

• So < collisions per unit time

• Leads to < successful collisions

• Rate of reaction increases.

Effect of increasing pressure on rate of reaction.

• > particles per unit volume

• Particles are closer together

• > collisions per unit time

• Rate increases

effect of increasing concentration on rate of reaction.

• > particles per unit volume

• > collisions per unit time

• > successful collisions

• Increases rate.

Effects of increasing surface area on rate of reactions

• > surface area for reaction to take place

• > collisions per unit time

• > successful collisions

• Increases rate.

Catalyst

• speed up reaction

• Does not get used up

• Provides alternative reaction pathway w/ lower E _act

what effects EQM position?

• Temperature

• Pressure

• Concentration

• NOT catalysts

What happens if you decrease the temperature of a reversible reaction that is exothermic in the forward direction?

• We favour the RHS forward reaction

• The exothermic reaction

• To oppose decrease in Temperature

• Yield of products increases

• A new equilibrium is established

What happens if you increase the pressure for the following reversible reaction?

N₂ + 3H₂ —2NH₃

• Yield of product increases

• Reaction favours the forward reaction on RHS

• Because pressure favours the side w/ fewer moles

• To counteract the increase in pressure

• A new equilibrium is established.

Effect of catalyst

• no effect on yield

• Speeds up both forward and backward direction at the same rate

• The equilibrium position stays uneffected / same

What is the effect of increasing A's concentration, on the yield of products in the following equation

A+B —— C+D

• yield of C + D increases

• Reaction favours RHS forward reaction

• To reduce concentration of A

• To counteract increase of A’s concentration

• A new equilibrium is established.