Graph 1 shows the decrease in the amount of a solid reactant with time. The graph is curved, becoming less steep because the reactants are being used up, so the speed decreases. In the first few minutes the graph will (i) decline less steeply for larger ‘lumps’ and (ii) decline more steeply with a fine powder o time (min) i.e., (i) less surface area gives slower reaction and (ii) more surface area a faster reaction.
Graph 2 shows the increase in the amount of a solid product with time. The graph tends towards a maximum amount possible when all the solid reactant is used up and the graph becomes horizontal. This means the speed has become zero as the reaction has stopped.
Graph 3 shows the decrease in reaction time with increase in temperature as the reaction speeds up. The reaction time can represent how long it takes to form a fixed amount of gas in the first few minutes of a metal carbonate-acid reaction, or the time it takes for so much sulphur to form In tin sodium thiosulphate-hydrochloric acid reaction.
Graph 4 shows the increase in speed of a reaction with increase in temperature as the particles have more and more kinetic energy. The rate of reaction is proportional to lit, where tis the reaction time.
Graph 5 shows the increase in the amount of a gas formed in a reaction with time. Again, the graph becomes horizontal as the reaction stops when one of the reactants is all used up!
Graph 6 shows the effect of Increasing concentration, which decreases the reaction time, as the speed increases because the greater the concentration the greater the chance of fruitful collision.
Graph 7 shows the rate/speed of reaction is often proportional to the concentration of one particular reactant. Rate This is due to the chance of a fruitful collision forming products being proportional to the concentration.