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The rate constant for a second order reaction, $\mathrm{A} \rightarrow$ Product is $1 \cdot 62 \mathrm{M}^{-1} \mathrm{~s}^{-1} .$ What will be the rate of reaction when concentration of reactant is $2 \times 10^{-3} \mathrm{M} ?$
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The correct answer is:
$6 \cdot 48 \times 10^{-6} \mathrm{Ms}^{-1}$
A $\longrightarrow$ Product
second order zeaction $R=K[A]^{2}$
$\begin{aligned}
\therefore \quad K &=1.62 \mathrm{M}^{-1} \mathrm{~S}^{-1} \\
[A] &=2 \times 10^{-3} \mathrm{M} \\
R &=\text { ? } \\
\longrightarrow \text { Rate of Reaction } R &=(1.62)\left(2 \times 10^{-3}\right)^{2} \\
&=6.48 \times 10^{-6} \mathrm{MS}^{-1}
\end{aligned}$
second order zeaction $R=K[A]^{2}$
$\begin{aligned}
\therefore \quad K &=1.62 \mathrm{M}^{-1} \mathrm{~S}^{-1} \\
[A] &=2 \times 10^{-3} \mathrm{M} \\
R &=\text { ? } \\
\longrightarrow \text { Rate of Reaction } R &=(1.62)\left(2 \times 10^{-3}\right)^{2} \\
&=6.48 \times 10^{-6} \mathrm{MS}^{-1}
\end{aligned}$
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