For the reaction $R \rightarrow P$,the concentration of a reactant changes from $0.03 \, M$ to $0.02 \, M$ in $25 \, minutes$. Calculate the average rate of reaction using units of time both in $minutes$ and $seconds$.
The average rate of reaction is given by the formula: $\text{Average rate} = -\frac{\Delta[R]}{\Delta t}$
Substituting the given values:
$\text{Average rate} = -\frac{[R]_2 - [R]_1}{t_2 - t_1} = -\frac{0.02 \, M - 0.03 \, M}{25 \, min} = -\frac{-0.01 \, M}{25 \, min} = 4 \times 10^{-4} \, M \, min^{-1}$
To convert the rate into $seconds^{-1}$:
$\text{Average rate} = \frac{4 \times 10^{-4} \, M}{60 \, s} = 6.67 \times 10^{-6} \, M \, s^{-1}$
Substituting the given values:
$\text{Average rate} = -\frac{[R]_2 - [R]_1}{t_2 - t_1} = -\frac{0.02 \, M - 0.03 \, M}{25 \, min} = -\frac{-0.01 \, M}{25 \, min} = 4 \times 10^{-4} \, M \, min^{-1}$
To convert the rate into $seconds^{-1}$:
$\text{Average rate} = \frac{4 \times 10^{-4} \, M}{60 \, s} = 6.67 \times 10^{-6} \, M \, s^{-1}$
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