The rate equation for the reaction $2 A+B \longrightarrow$ products is rate $=k[A][B]^2$. If $k$ at $T(\mathrm{~K})$ is $5.0 \times 10^{-6} \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$, the initial rate of the reaction, when $[A]=0.05 \mathrm{~mol} \mathrm{~L}^{-1}$ and \([B]=0.1…

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The rate equation for the reaction $2 A+B \longrightarrow$ products is rate $=k[A][B]^2$. If $k$ at $T(\mathrm{~K})$ is $5.0 \times 10^{-6} \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$, the initial rate of the reaction, when $[A]=0.05 \mathrm{~mol} \mathrm{~L}^{-1}$ and $[B]=0.1 \mathrm{~mol} \mathrm{~L}^{-1}$ is

Aicharya · Accepted Answer

For the reaction, $2 A+B \longrightarrow$ Products $\text {Rate }=k[A][B]^2$ Given, Rate constant, $k$ of reaction $=5.0 \times 10^{-6} \mathrm{~mol}^{-2} \mathrm{~L}^2 \mathrm{~s}^{-1}$ $\begin{aligned} {[A]=0.05 \mathrm{~mol} \mathrm{~L}^{-1} } \ {[B]=0.1 \mathrm{~mol} \mathrm{~L}^{-1} } \end{aligned}$ $\begin{aligned} \therefore \text { Rate of reaction } & =5.0 \times 10^{-6}[0.05][0.1]^2 \ & =5 \times 10^{-6} \times 5 \times 10^{-4} \ & =2.5 \times 10^{-9} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \end{aligned}$

The rate equation for the reaction \(2 A+B \longrightarrow\) products is rate \(=k[A][B]^2\). If \(k\) at…

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