Question

Given the initial rate data for the reaction being A + B --> D determine the rate expression for the reaction and the (k) rate constant. (The units of [A] [B] are moles/liter and the units of IRR is moles/liter seconds). If the [A]=[B]=.030M, what would the IRR be?

                        [A]                  [B]                   IRR

                        0.020               0.010               .028

                        0.020               0.020               .224

                       

0.020               0.040               1.792

40.                0.020               .448

.010                 0.020               .056

Answer 1

Dear Student,

[A]                  [B]                   IRR

0.020               0.010               .028

0.020               0.020               .224

0.020               0.040               1.792

0.020               .448

.010                 0.020               .056

Rate =[A]^x*[B]^y

For finding the x value we have to consider two trails where [B] is constant; that will be (2)& (5)

[[0.020]/[0.010]]^x= 0.224/0.056

2^x=4 => 2^x=2²=> x=2

Similarly,For finding the y value we have to consider two trails where [A] is constant; that will be (1)& (2)

[0.02]/[0.01]]^y=0.22/0.028=7.85 approx 8

2^y=8=> 2^y=2³

y=3

Therefore,Rate= [A]²*[B]³

If [A]=[B]=0.30

IRR= [0.30]²*[0.30]³ =0.00243 moles/liter

Thanks & Best Wishes