The stoichiometric equation for a reaction is A + B -> C + D. The initial rate o

Question

The stoichiometric equation for a reaction is A + B -> C + D. The initial rate of formation of C is measured with the following results: What is the order of the reaction with respect to A? What is the order of the reaction with respect to B? Use your conclusion in parts (a) and (b) to write a differential equation for the appearance of What is the rate constant k for the reaction? Do not omit the units of k. Give a possible mechanism for the reaction and discuss in words, or give equations, to show how the mechanism is consistent with the experiment.

Explanation / Answer

1. a) order w.r t to A

(1/2)^n = ((1.0*10^(-3))/(4.0*10^(-3)))

n =2

order w.r t to A = 2

b) order w.r t to B = 0

(1/2)^n = ((1.0*10^(-3))/(1.0*10^(-3)))

n = 0

total order = 2+0   = 2

c) rate = -d[A]^2/dt = -d[B]^0/dt = +d[C]/dt

d) K= x/t(a-x)a = M-1.S-1.

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