For the reaction R P, the concentration of a reactant changes from 0.03 to 0.22 M in 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.

Question

4 Answers

kritika · Answer 1 · 2021-12-23T03:22:14+0000

Average rate =

$-\left[\frac{\text { Final concentration }-\text { Initial concentration }}{\text { Time interval }}\right]$

$=-\frac{\Delta[\mathrm{R}]}{\Delta \mathrm{t}}$

$=-\left[\frac{\left[\mathrm{R}_{2}\right]-\left[\mathrm{R}_{1}\right]}{\mathrm{t}_{2}-\mathrm{t}_{1}}\right]=-\left[\frac{0.02-0.03}{25}\right]$

$=-\left[\frac{-0.01}{25}\right]$ Average rate

$=4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$

$4 \times 10^{-4}$

$60 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$

$=6.66 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ Hence average rate

$=4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$ Average rate

$=6.66 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$

$4 \times 10^{-4}$
60 mol

$L^{-1} S^{-1}$

$=6.66 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$
Hence average rate

$=4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$
Average rate

$=6.66 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$