The hypothesis was supported as the rate of reaction did increase as the concentration and the temperature increased. The concentration, or molarity, of the reactants increased in relation to time in the form M=1.1541e0.0016t. This is an accurate relationship as the volume remains the same as the number of molecules increase, thus the rate would increase exponentially as the molecules collide at a constant growth rate. This is also a reliable model as the R² value is 0.9697. The hypothesis that the reaction would be first order was also supported, which can be seen in graph 2 of the results, where the natural log of the molarity was plotted against time and the trendline was linear, with the equation of ln(M) = 0.0016t + 0.1434. This is because if a relationship is first order, it would only have to be integrated once before the form is linear. Since our graph did form a linear plot after a single integration was performed, the relationship is accurate and supports the hypothesis that the rate was first order. The R² value was 0.9697 and again supports that the model is accurate.

Again, the hypothesis that the relationship between temperature and time would be based on Arrhenius’ equation, and that the rate of reaction increases as temperature increases was supported. Time was plotted against temperature (see graph 3 of results), and the relationship found was a high power equation, T = 323.11t-0.03, where the time taken for a reaction to take place increases drastically…