Question

A) 2A → B + C

The above reaction is run and it is found that a plot of the concentration of A versus time is linear as the reaction proceeds. This indicates that the reaction is ...

		zero order in [A]
		first order in [A]
		second order in [A]
		third order in [A]

B)2A → B + C

The above reaction is run and it is found that a plot of the natural log of the concentration versus time is linear. This indicates that the reaction is ...

		zero order in [A]
		first order in [A]
		second order in [A]
		third order in [A]

Answer 1

This reaction is zero order since the data only fits to zero order integrated rate law.

Integrated rate law:

[A] = [A]₀ – kt

Here y = [ A] and slope is -k , so when we plot concentration of A with respect to t then we get the equation in the form of line

y = mx + c

So the answer Zero order in [A]

B)

This reaction fits to first order reaction

Integrated rate equation for first order rate law.

ln [A]_t = ln [A]₀ -kt

when we plot ln [A]_t Vs t then we get straight line.

So answer is :

First order with respect to A