Chemical Kinetics

Question

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For the reaction R → P, the concentration of a reactant changes from 0.03 M to 0.02 M is 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.

Solution

Given that
Initial concentration, [R1] = 0.03
Final concentration, [R2] = 0.02
Time taken ∆t = 25 min = 25 × 6 0 = 1500 sec (1 min = 60 sec )
The formula of average rate of change

r_{av} = \frac{- ∆ R}{∆ t} = \frac{∆ [P]}{∆ t}

(i) Average rate

= \frac{(0.03 - 0.02) M}{25 \times 60 \sec} = \frac{0.01 M}{25 \times 60 s} = 6.66 M s^{- 1}

(ii) Average rate

= \frac{(0.03 - 0.02) M}{25 \min} = \frac{0.01 M}{25} = 0.0004 {Ms}^{- 1} .

Some More Questions From Chemical Kinetics Chapter

The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?

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Chemical Kinetics

For the reaction R → P, the concentration of a reactant changes from 0.03 M to 0.02 M is 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.

Some More Questions From Chemical Kinetics Chapter

The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?

What will be the effect of temperature on rate constant?

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