A reaction is of first order with respect to reactant [A] and second order with regard to reactant…
A reaction is of first order with respect to reactant [A] and second order with regard to reactant [B]. What is the effect on rate of reaction when:
(i)[1.0]
concentration of only [B] is increased three times?
(ii)[1.0]
concentration of both [A] and [B] is doubled?
Answer
Answer (i)
AIWritten by AI (gemini) - it can contain mistakes.
The rate law is $\text{Rate} = k[\text{A}][\text{B}]^2$.
When $[\text{B}]$ is increased three times:
$\text{Rate}' = k[\text{A}](3[\text{B}])^2 = 9 k[\text{A}][\text{B}]^2 = 9 \times \text{Rate}$
The rate of reaction increases by 9 times (becomes 9 times the initial rate).
Answer (ii)
AIWritten by AI (gemini) - it can contain mistakes.
When both $[\text{A}]$ and $[\text{B}]$ are doubled:
$\text{Rate}' = k(2[\text{A}])(2[\text{B}])^2 = 8 k[\text{A}][\text{B}]^2 = 8 \times \text{Rate}$
The rate of reaction increases by 8 times (becomes 8 times the initial rate).
From ISC 2026 Chemistry Paper 1, question 2.