Students perform an investigation of the reaction
A(g) + B(g) → C(g)
at 290 K and at 310 K. The rate law is known to be rate = k[A][B]. All concentrations are kept the same in both trials. Based on literature data the rate constant at 310 K is expected to be 6.0 times larger than at 290 K, yet the class observes only a 2.5-fold increase in the rate.
(a) Propose two plausible experimental factors, other than measurement error, that could reduce the observed temperature effect on the rate by altering the fraction of properly oriented collisions.
(b) For one of the factors proposed in part (a), design a modification to the experimental setup that would allow you to test whether that factor is responsible for the discrepancy.
(c) Predict qualitatively how your modification in part (b) would change the measured rate at 310 K if the hypothesis is correct, and explain your reasoning.
(d) Describe how you would analyze the new data to decide whether the discrepancy was indeed caused by the factor investigated.