Q. The data for the reaction, A+B→C [table] Ex | $\lbrack A\rbrack_{0}$ | $\lbrack B\rbrack_{0}$ | Initial rate ; 1 | 0.012 | 0.035 | 0.10 ; 2 | 0.024 | 0.070 | 0.80 ; 3 | 0.024 | 0.035 | 0.10 ; 4 | 0.012 | 0.070 | 0.80 [/table] The rate law corresponds to the above data is
A) $rate = k\lbrack B\rbrack^{3}$
B) $rate = k\lbrack B\rbrack^{4}$
C) $rate = k\lbrack A\rbrack\lbrack B\rbrack^{3}$
D) $rate = k\ \lbrack A\rbrack^{2}\lbrack B\rbrack^{2}$
Explanation
(c)
For the reaction,
A+B →C
$Rate = k\lbrack A\rbrack_{0}^{x}.\lbrack B\rbrack_{0}^{y}$
$\frac{Rate_{2}}{Rate_{3}} = \frac{k(0.024)^{x}(0.070)^{y}}{k(0.024)^{x}(0.035)^{y}} = \frac{0.80}{0.10}$
$(2)^{y} = 8$
$y = 3$
$\frac{Rate_{3}}{Rate_{1}} = \frac{k(0.024)^{x}(0.035)^{y}}{k(0.012)^{x}(0.035)^{y}} = \frac{0.10}{0.10}$
$(2)^{x} = 1$
$x = 0$
$Rate = k\lbrack B\rbrack^{3},\$where, k=rate constant
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.