If the rate law for this reaction is, Rate = k [NO(g)] 2 [H 2 (g)], what is the

Question

If the rate law for this reaction is, Rate = k [NO(g)]2 [H2(g)], what is the value of the rate constant?

a) The value of rate constant is k = 2.82e+05 M-2 s-1.
b) The value of rate constant is k = 1.54e+04 M-2 s-1.
c) The value of rate constant is k = 1.12e+05 M-2 s-1.
d) The value of rate constant is k = 7.82e+05 M-2 s-1.
e) The value of rate constant is k = 4.01e+04 M-2 s-1.

Experiment [NO(g)] (M) [H2(g)] (M) Rate (M/s) 1 0.0827 0.0827 6.33e+01 2 0.0827 0.165 1.26e+02 3 0.165 0.0827 2.52e+02 4 0.165 0.165 5.03e+02

Explanation / Answer

Answer: C

Rate = k * [NO]^a * [H2]^b

Exp 1: 6.33e+01 = k * [0.0827]^a * [0.0827]^b
Exp 2: 1.26e+02 = k * [0.0827]^a * [0.1650]^b
Exp 3: 2.52e+02 = k * [0.1650]^a * [0.0827]^b
Exp 4: 5.03e+02 = k * [0.1650]^a * [0.1650]^b

Exp2/Exp1 --> 2 = 2^b => b = 1
Exp3/Exp1 --> 4 = 2^a => a = 2

6.33e+01 = k * [0.0827]^2 * [0.0827]^1
k = 6.33e+01/(0.0827)^3 = 1.12e+05 M-2 s-1

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