1. What is the order of reaction with respect to A? 2. What is the order of reac

Question

1. What is the order of reaction with respect to A? 2. What is the order of reaction with respect to B? below: The initial rate of the reaction A + 3B 2C + D was determined for different initial conditions as shown initial rate, M/s 3.35 x 104 1.35 x 10-3 6.75 x 10 4 2.70 x 10-3 Experiment # 1 [A], M | [B], M 0.185 0.185 0.370 0.370 0.133 0.266 - 0.133 0.266 What is the order of reaction with respect to A? 2. What is the order of reaction with respect to B 3. What is the value of the rate constant, k? [note: don't forget your units

Explanation / Answer

A + 3B -----> 2C +D

Rate is directly proportioal to concenteration

Rate= k[A]^x [B]^y

where x and y are the order of reaction with respect to A and B

Dividing the values of experiment 1 and 2, we get

Rate 2/ rate 1=   [A]2^x[B]2^y/[A]1^x[B]1^y

1.35 x 10^-3/3.35 x 10^-4= [0.185]^x [0.266]^y/[0.185]^x [0.133]^y

4.0= (2)^y

(2)^2=(2)^y

y=2

Dividing the values of expt 3 by 1

Rate 3/rate 1= [A]3^x[B]3^y/[A]1^x[B]1^y

6.75 x 10^-4/ 3.35 x 10^-4 = [0.370]^x[0.133]^y / [0.185]^x[0.133]^y

2 = (2)^x

x=1

So rate of reaction with respect to A is 1 and B is 2

Rate= k[A]^x[B]^y

3.35 x 10^-4= k(0.185)^1. (0.133)^2

k= 3.35 x 10^-4/ 3.27 x 10^-3= 0.102 mol-2 L^2min-1

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