Question

Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of...

Consider the reaction

A+2B⇌C

whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table:

Trial [A]
(M)		 [B]
(M)		 Rate
(M/s)
1 0.15 0.010 2.7×10−4
2 0.15 0.020 5.4×10−4
3 0.30 0.010

1.1×10−3

Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M.

Express your answer to two significant figures and include the appropriate units.

Science   Chemistry   
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Homework Answers

Answer #1

see experiment 1 and 3:

[A] doubles

[B] is constant

rate becomes 4 times

so, order of A is 2

see experiment 1 and 2:

[A] is constant

[B] doubles

rate doubles

so, order of B is 1

overall order = 2 + 1 = 3

Rate law is:

rate = k*[A]^2*[B]

Put values from 1st row of table in rate law

rate = k*[A]^2*[B]

2.7*10^-4 = k*0.15^2*0.01^1

k = 1.2 M-2.s-1

Now put all values to find rate at given concentration

rate = k*[A]^2*[B]

rate =1.2*0.5^2*0.075

rate = 0.0225 M/s

Answer: 2.2*10^-2 M/s

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