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A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is \((i)\) doubled (ii) reduced to half?
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Let concentration of the reactant be \([\mathrm{A}]=\mathrm{a}\) Rate \(=k[\mathrm{~A}]^2=k a^2\)
(i) If \([\mathrm{A}]=2 a\), rate \(=k(2 a)^2=4 k a^2=4\) times.
(ii) If \([\mathrm{A}]=a / 2\), rate \(=k\left(\frac{a}{2}\right)^2=\frac{1}{4} k a^2=\frac{1}{4}\) th.
(i) If \([\mathrm{A}]=2 a\), rate \(=k(2 a)^2=4 k a^2=4\) times.
(ii) If \([\mathrm{A}]=a / 2\), rate \(=k\left(\frac{a}{2}\right)^2=\frac{1}{4} k a^2=\frac{1}{4}\) th.
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