Question

$nA\to$ product $\frac{dx}{dt}=k{\left[A\right]}^n$ For the reaction, rate constant and rate of the reaction are equal, then on doubling the concentration of $A,$ rate becomes,

• A. four times
• B. halved
• C. constant
• D. doubled

Answer 1

Answer: (C)

$\left(\frac{dx}{dt}\right)=k{\left[A\right]}^x$
$\left(\frac{dx}{dt}\right)=k{\left[A\right]}^0=k$
rate = rate constant
Thus, order = zero
Rate is independent of concentration of $A.$Thus, rate remains constant