The data in the table below were obtained for the reaction: 2 ClO_2(aq) + 2 OH^-

Question

The data in the table below were obtained for the reaction: 2 ClO_2(aq) + 2 OH^- (aq) rightarrow ClO_3^- (aq) + ClO_2^- (aq) + H_2O (l) What is the order of the reaction with respect to ClO_2? A) 4 B) 1 C) 0 D) 2 What is the order of the reaction with respect to OH^-? A) 0 B) 1 C) 2 D) 3 What is the overall order of the reaction? A) 0 B)1 C) 4 D) 3 What is the magnitude of the rate constant for the reaction? A) 115 B) 1.15 times 10^4 C) 713 D) 4.6 For a first-order reaction, a plot of _______ versus _____________ A) ln [A]_t, t B) 1/[A]_t, t C) ln [A]_t, 1/t D) [A]_t, t

Explanation / Answer

Let us take the rate expression as

rate = k [ClO2]x [OH-]y  where x and y are orders with respect to ClO2 and Oh- respectively.

9) Comparing rate 1 and rate2 where [OH-] is constant

0.0248/0.00276 = [0.060/0.020]x

   which give s 9 = 3x or x = 2

That is order with respect to CLO2 = 2

10) similarlycomparing 2 and 3 rates where [ClO2] = constant

0.00828/0.00276 = [0.090/0.30]y  or 3 = 3y , thus y =1

thus order with respect to OH- = 1

11) overall order of reaction = 2 +1 = 3

12) the rate constant of the reaction is calculate by substituting the gives cvalues of rate and concentration in the rate expression

rate = k [ClO2]2[Oh-]

for experiment 1 k = 229

for experiment 2 , k = 230

for experiment 3 , k = 230.

Thus average value of k = 229.7

But no option matches this

13) First order rate law is

[A]t  = [A]0 e-kt

in logarithmic form ln[A]t = -kt +.ln[A]o

it is of the form y = mx

So a graph between ln[A]t and t will be a straight line with negative slope of -k

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