For the reaction A+B+C?D+E, the initial reaction rate was measured for various i

Question

For the reaction A+B+C?D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected:

What is the value of the rate constant k for this reaction?

Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.

Trial [A]
(M) [B]
(M) [C]
(M) Initial rate
(M/s) 1 0.20 0.20 0.20 6.0×10?5 2 0.20 0.20 0.60 1.8×10?4 3 0.40 0.20 0.20 2.4×10?4 4 0.40 0.40 0.20 2.4×10?4

Explanation / Answer

see experiment 1 and 3:

[A] doubles

[B] is constant

[C] is constant

rate becomes 4 times

so, order of A is 2

see experiment 3 and 4:

[A] is constant

[B] doubles

[C] is constant

rate is constant

so, order of B is 0

see experiment 1 and 2:

[A] is constant

[B] is constant

[C] becomes 3 times

rate becomes 3 times

so, order of C is 1

Rate law is:

rate = k [A]^2[B]

put values from experiment 1

6.0*10^-5 M/s = k (0.20 M)^2 (0.20 M)

6.0*10^-5 M/s = k 0.008 M^3

K = 7.5*10^-3 M-2.s-1

Answer:

7.5*10^-3

M-2.s-1

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