Question

For the given reaction,
$3A+2B\to C+D,$ the experimental rate law is $R=K\left[A\right][B{]}^2$. When the active mass of 'B' is kept constant and 'A' is doubled then, the rate of the reaction will

• A. increases by 4 times
• B. increases by 2 times
• C. decreases by 4 times
• D. decreases by 2 times

Answer 1

The correct option is B increases by 2 times

For the given reaction, the experimental rate law is,
$Rate=K\left[A\right]{\left[B\right]}^2$

When the concentration of 'A' is doubled (2A) and 'B' is kept constant,

$Rate=K{\left[2A\right]}^1{\left[B\right]}^2$$=2K\left[A\right][B{]}^2$

Thus, the rate of reaction is increased by 2 times.