For the reaction A + 2 B + C 3 D + 2 F the following experimental data were obta
ID: 984656 • Letter: F
Question
For the reaction
A + 2 B + C 3 D + 2 F
the following experimental data were obtained.
Experiment
[A] (M)
[B] (M)
[C] (M)
Rate (M/min)
1
0.10
0.10
0.10
2.0 x 10-5
2
0.10
0.10
0.30
6.0 x 10-5
3
0.20
0.10
0.10
8.0 x 10-5
4
0.10
0.40
0.10
2.0 x 10-5
Part #1:
Which represents the correct rate law?
A) Rate = k [A]0[B]2[C]
B) Rate = k [A]2[B]0[C]
C) Rate = k [A]1[B]2[C]1
D) Rate = k [A]0[B]2[C]1
E) Rate = k [A]1[B]2[C]0
Part #2:
Which represents the correct units of the rate constant k for this reaction?
A) 1/s
B) M/s
C) M4/s
D) 1/M2s
Part #3:
What is the value of the rate constant k for this reaction?
Experiment
[A] (M)
[B] (M)
[C] (M)
Rate (M/min)
1
0.10
0.10
0.10
2.0 x 10-5
2
0.10
0.10
0.30
6.0 x 10-5
3
0.20
0.10
0.10
8.0 x 10-5
4
0.10
0.40
0.10
2.0 x 10-5
Explanation / Answer
initial rates
rate1 / rate2 = ([A1][A2])^a([B1][B2])^b([C1][C2])^c
for C
2/ 6=1*([0.1/0.3)^c
C = 1
for A
rate1 / rate2 = ([A1][A2])^a
for C
2/ 8=1*([0.1/0.2)^a
1/4 = 1/2^a
A = 2
For B
rate1 / rate2 = ([A1][A2])^a
for B
2/2=1*(.1/.4)^b
b = 0
therefore
order:
rate = k*[A]^2[B]^0[C]^1
k must have units of
rate = mol/V-s
k = rate /([M/s]^2 * [M/s])
k = M/s / (M^3/s^2) = M^2 s
3)
k =
0.10
0.10
0.10
2.0 x 10-5
2*10^-5 = k*(0.1^2)(0)(0.1)
k = (2*10^-5 )/(0.1^3) = 0.02
0.10
0.10
0.10
2.0 x 10-5
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