Question

# Using the initial rates of reaction for the following reaction: A + 3B → 2C [A]...

Using the initial rates of reaction for the following reaction:

A + 3B → 2C

 [A] (mol/L) [B] (mol/L) Initial Rate (mol/L∙s) 0.210 0.150 3.41x10-3 0.210 0.300 1.36x10-2 0.420 0.300 2.73x10-2

What is the order of the reaction with respect to A?

What is the order of the reaction with respect to B?

The overall rate expression?___________________

Calculate the rate constant including the units.

Rate law = k [ A]m [B]n

K is rate constant , m and n are the order.

Lets find order by using different experimental runs.

 Exp No. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L∙s) 1 0.210 0.150 3.41x10-3 2 0.210 0.300 1.36x10-2 3 0.420 0.300 2.73x10-2

Lets take ratio of rate of exp 3:2 , then we will get order with respect A.

2.37 E-2 / 1.36 E-2 = ( .410/0.210)m

Lets find value of m

m = 1

so the order with respect to A is 1.

To get order with respect to B and for that we use ratio with 2 : 1 .

1.36 E-2/ 3.41 E-3 = (0.300 / 0.150 )n

Lets calculate n

n = 1.99 = 2

order with respect to B = 2

so the rate law becomes

Rate= k [A][B]2

Lets use extp 1 to get k

Rate= k [A][B]2

3.41 E-3 = k (0.210)x(0.150)2

k = 0.72 L mol-1 sec-1

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