Question

For the reaction $A+B\to C$, determine the order of the reaction with respect to $B$ from the information given below.

${\left[A\right]}_{\circ }$	${\left[B\right]}_{\circ }$	Initial rate (M/s)
1.00	1.00	2.0
1.00	2.00	8.1
2.00	2.00	15.9

• A. Zero order
• B. First order
• C. Second order
• D. Third order
• E. Fourth order

Answer 1

The correct option is C Second order

Analyzing first and second raw,when concentration of $B$ is doubled then initial rate increased by four times,so it is increasing by square of concentration.Hence it is a second order reaction.

$Rate$$=$$k\left[A{]}^x\right[B{]}^2$ Using this rate expression and keeping $\left[A\right]$ constant,if we double $\left[B\right]$ then rate increases four times.