The reaction below is investigated in a well-stirred batch reactor at 298 K.
Overall reaction: A(g) + 2B(g) → products
Kinetic studies suggest the following mechanism:
Step 1 (slow): A(g) + B(g) → E(g)
Step 2 (fast): E(g) + B(g) → products
(a) Show that the mechanism is consistent with a second-order overall rate law and specify its form in terms of concentrations.
(b) Derive a general algebraic expression that predicts how the initial rate will change when [A] is multiplied by m and [B] is multiplied by n (where m and n are positive real numbers).
(c) Using the expression in part (b), calculate the exact factor change in initial rate when [A] is doubled and [B] is quadrupled.
(d) The reactor operator mistakenly believes that halving [B] will have a smaller effect on the rate than halving [A]. Use your expression from part (b) to evaluate this claim quantitatively and comment on its validity.
(a) Demonstrate that the mechanism yields a second-order overall rate law and state that law explicitly.
(b) Derive a general expression for the factor change in initial rate when [A] is multiplied by m and [B] by n.
(c) Calculate the factor change when [A] is doubled and [B] is quadrupled.
(d) Assess the operator’s claim by comparing the effect of halving [B] with halving [A] using your expression from part (b).