Experiment Initial [A) (mol/L) Initial [B] (mol/L) Initial [C] (mol/L) Initial R
ID: 939489 • Letter: E
Question
Experiment
Initial [A)
(mol/L)
Initial [B]
(mol/L)
Initial [C]
(mol/L)
Initial Rate(mol/L-s)
1
0.0500
0.0500
0.0100
6.25 x 10-3
2
0.100
0.0500
0.0100
1.25 x 10 -2
3
0.100
0.100
0.0100
5.00 x 10-2
4
0.0500
0.0500
0.0200
6.25 x 10-3
The above data were obtained at constant temperature. Pick the best expression for the rate law for the reaction:
a) k[A][B][C]
b) k [A]2[B][C]
Experiment
Initial [A)
(mol/L)
Initial [B]
(mol/L)
Initial [C]
(mol/L)
Initial Rate(mol/L-s)
1
0.0500
0.0500
0.0100
6.25 x 10-3
2
0.100
0.0500
0.0100
1.25 x 10 -2
3
0.100
0.100
0.0100
5.00 x 10-2
4
0.0500
0.0500
0.0200
6.25 x 10-3
Explanation / Answer
order w.r.t A = 1
(6.25*10^(-3)/(1.25*10^(-2))) = (0.05/0.1)^n
n = 1
order w.r.t B = 2
(1.25*10^(-2)/(5*10^(-2))) = (0.05/0.1)^n
n = 2
order w.r.t C = 0
(6.25*10^(-3)/(6.25*10^(-3))) = (0.01/0.02)^n
n = 0
RATE = k[A]^1[B]^2[C]^0
(6.25*10^(-3)) = k(0.05^1*0.05^2*0.01^0)
k = 50 M-2.s-1
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