kinetics and equilibria

rate of reaction equation

change in amount of substance/ time or the gradient of the line

methods of monitoring rate of reaction

measure mass lost as gas is evolved or measure time taken for a certain volume of gas to be given off

how does SA affect rate

a greater SA means more successful collisions per second, decreasing the size of the particles increases the SA, this increases the area of contact so rate of reaction increases

how does concentration affect rate

increasing concentration causes more particles to be in the same volume, so more successful collisions per second so rate of reaction increases

how does pressure affect rate

an increase in pressure causes the molecules to be forced closer together so concentration increases meaning more successful collisions per second and so rate of reaction increases

homogenous catalyst definition

a catalyst thats in the same physical state as the reactants

heterogenous catalyst

a catalyst thats in a different physical state to the reactants

dynamic equilibrium definition

a system where the rate of the forward reaction is equal to the rate of the backwards reaction

so no overall change in concentrations of products or reactants

must be a closed system

what happens to equilibrium if concentration of the reactant increases

it shifts to the right

what happens to equilibrium if concentration of the product increases

it shifts to the left

whats the effect of temp on equilibrium

an increase in temp causes equilibrium to shift to minimize change

it favours the endothermic reaction

whats the effect of pressure on equilibrium

an increase in pressure causes equilibrium to shift to the side with the fewest gas molecules

whats the effect of a catalyst on equilibrium

no effect on position of equilibrium

rate of forward and backward reactions increases as catalysts provide an alternative path of lower activation energy so higher proportion of successful collisions

whats the KC equation

(products/reactants)