Given the reaction: 2A + 2B C + 3D and the following initial rates data: Expt [A

ID: 884803 • Letter: G

Question

Given the reaction: 2A + 2B C + 3D and the following initial rates data:

Expt

[A]

[B]

Rate of Formation of C

2.00 M

2.40 Ms-1

2.00 M

6.00 M

64.80 Ms-1

8.00 M

2.00 M

9.60 Ms-1

a. Determine and write the rate-law expression for this reaction to include the numerical value and units for k. Circle your final answer.)

b. The reaction is _______order in A, _______order in B, and _______order overall.

Expt

[A]

[B]

Rate of Formation of C

2.00 M

2.40 Ms-1

2.00 M

6.00 M

64.80 Ms-1

8.00 M

2.00 M

9.60 Ms-1

a)
let rate law be:
rate = K [A]^x * [B]^y
considering experiment 1:
2.4 = K [2]^x * [2]^y

considering experiment 2:
64.8 = K [2]^x * [6]^y

considering experiment 3:
9.6 = K [8]^x * [2]^y

divide 2nd eqn by 1st eqn:
64.8/2.4 = (6/2)^y
27= 3^y
3^3= 3^y
so, y= 3

divide 3rd eqn by 1st eqn:
9.6/2.4 = (8/2)^x
4= 4^x
so, x= 1

putting the value of x and y in 1st eqn
2.4 Ms-1 = k*(2M)^1 (2M)^3
k = 0.3 M-3S-1

Rate = (0.3 M-3S-1) [A] [B]^3

b)
The reaction is 1st order in A, 3rd order in B, and 4th order overall.

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