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  • The concentration of reactant changes from 0.03 M to 0.02 M in 25 min. Calculate the average rate of reaction using units of time in seconds?Option: 1<

The concentration of reactant changes from 0.03 M to 0.02 M in 25 min. Calculate the average rate of reaction using units of time in seconds?

Option: 1

6.67 \times 10^{-6} \mathrm{\: mol\: } \mathrm{L}^{-1} \mathrm{s}^{-1}


Option: 2

0.4 \times 10^{-5} \mathrm{\: mol\: } \mathrm{L}^{-1} \mathrm{s}^{-1}


Option: 3

0.4 \times 10^{-3} \mathrm{\: mol} \mathrm{\: L}^{-1} \mathrm{s}^{-1}


Option: 4

0.11 \times 10^{-5} \mathrm{\: mol\: } \mathrm{L}^{-1} \mathrm{s}^{-1}


Answers (1)

best_answer

As we have learnt, 

\mathrm{Rate\ of\ Reaction = -\frac{Change\ in\ concentration\ of\ reactant}{time}}

 

\text { Rate }=\mathrm{\frac{-\Delta [R]}{\Delta t}}=\frac{[0.03 \mathrm{\: M}-0.02 \mathrm{\: M}]}{25 \mathrm{\: min}}
             \begin{array}{l}{=0.01 / 25 \mathrm{\: mol} \mathrm{\: L}^{-1} \mathrm{min}^{-1}} \\ {=0.4 \times 10^{-3} \mathrm{\: mol} \mathrm{\: L}^{-1} \mathrm{min}^{-1}} \\ {=0.4 \times 10^{-3} \mathrm{\: mol} \mathrm{\: L}^{-1} \mathrm{min}^{-1} \mathrm{min} / 60 \mathrm{s}} \\ {=6.67 \times 10^{-6} \mathrm{mol} \mathrm{\: L}^{-1} \mathrm{s}^{-1}}\end{array}

Therefore, option(1) is correct

Posted by

Divya Prakash Singh

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