320360
For a first order reaction, the half-life is 10 mins. How much time in minutes will it take to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration?
1 10
2 20
3 30
4 40
Explanation:
It takes two half-lives to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration.
Hence, total time taken \({\mathrm{=10+10}}\) \(=20 \text { minutes }\)
CHXII04:CHEMICAL KINETICS
320361
For a first order reaction, the time taken to reduce initial concentration by a factor of 1/4 is 10 minutes. The time required to reduce initial concentration by a factor 1/16 will be
320362
In a first order reaction concentration of reactant decreases from \({\text{20 m mol}}\) to \({\text{10 m mol}}\) in \(1.151 \mathrm{~min}\). What is rate constant?
320363
Number of average life times \(\left( {{{\rm{T}}_{{\rm{av}}}}} \right)\) required for a first order reaction to achieve 99.9% level of completion is
1 6.9
2 1.5
3 0.105
4 9.2
Explanation:
Time required for \(99.9 \%\) reaction is 10 times of half-life period. \(t_{99.9}=10 t_{50}\) But \(t_{50}=\dfrac{0.693}{k}\) \(\therefore \quad T_{a v}=\dfrac{1}{k}\) and \(t_{50}=0.693 T_{a v}\) \(\therefore \quad t_{99.9}=10 \times 0.693 T_{a v}=6.93 T_{a v}\)
320360
For a first order reaction, the half-life is 10 mins. How much time in minutes will it take to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration?
1 10
2 20
3 30
4 40
Explanation:
It takes two half-lives to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration.
Hence, total time taken \({\mathrm{=10+10}}\) \(=20 \text { minutes }\)
CHXII04:CHEMICAL KINETICS
320361
For a first order reaction, the time taken to reduce initial concentration by a factor of 1/4 is 10 minutes. The time required to reduce initial concentration by a factor 1/16 will be
320362
In a first order reaction concentration of reactant decreases from \({\text{20 m mol}}\) to \({\text{10 m mol}}\) in \(1.151 \mathrm{~min}\). What is rate constant?
320363
Number of average life times \(\left( {{{\rm{T}}_{{\rm{av}}}}} \right)\) required for a first order reaction to achieve 99.9% level of completion is
1 6.9
2 1.5
3 0.105
4 9.2
Explanation:
Time required for \(99.9 \%\) reaction is 10 times of half-life period. \(t_{99.9}=10 t_{50}\) But \(t_{50}=\dfrac{0.693}{k}\) \(\therefore \quad T_{a v}=\dfrac{1}{k}\) and \(t_{50}=0.693 T_{a v}\) \(\therefore \quad t_{99.9}=10 \times 0.693 T_{a v}=6.93 T_{a v}\)
320360
For a first order reaction, the half-life is 10 mins. How much time in minutes will it take to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration?
1 10
2 20
3 30
4 40
Explanation:
It takes two half-lives to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration.
Hence, total time taken \({\mathrm{=10+10}}\) \(=20 \text { minutes }\)
CHXII04:CHEMICAL KINETICS
320361
For a first order reaction, the time taken to reduce initial concentration by a factor of 1/4 is 10 minutes. The time required to reduce initial concentration by a factor 1/16 will be
320362
In a first order reaction concentration of reactant decreases from \({\text{20 m mol}}\) to \({\text{10 m mol}}\) in \(1.151 \mathrm{~min}\). What is rate constant?
320363
Number of average life times \(\left( {{{\rm{T}}_{{\rm{av}}}}} \right)\) required for a first order reaction to achieve 99.9% level of completion is
1 6.9
2 1.5
3 0.105
4 9.2
Explanation:
Time required for \(99.9 \%\) reaction is 10 times of half-life period. \(t_{99.9}=10 t_{50}\) But \(t_{50}=\dfrac{0.693}{k}\) \(\therefore \quad T_{a v}=\dfrac{1}{k}\) and \(t_{50}=0.693 T_{a v}\) \(\therefore \quad t_{99.9}=10 \times 0.693 T_{a v}=6.93 T_{a v}\)
320360
For a first order reaction, the half-life is 10 mins. How much time in minutes will it take to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration?
1 10
2 20
3 30
4 40
Explanation:
It takes two half-lives to reduce the concentration of reactant to \({\mathrm{25 \%}}\) of its original concentration.
Hence, total time taken \({\mathrm{=10+10}}\) \(=20 \text { minutes }\)
CHXII04:CHEMICAL KINETICS
320361
For a first order reaction, the time taken to reduce initial concentration by a factor of 1/4 is 10 minutes. The time required to reduce initial concentration by a factor 1/16 will be
320362
In a first order reaction concentration of reactant decreases from \({\text{20 m mol}}\) to \({\text{10 m mol}}\) in \(1.151 \mathrm{~min}\). What is rate constant?
320363
Number of average life times \(\left( {{{\rm{T}}_{{\rm{av}}}}} \right)\) required for a first order reaction to achieve 99.9% level of completion is
1 6.9
2 1.5
3 0.105
4 9.2
Explanation:
Time required for \(99.9 \%\) reaction is 10 times of half-life period. \(t_{99.9}=10 t_{50}\) But \(t_{50}=\dfrac{0.693}{k}\) \(\therefore \quad T_{a v}=\dfrac{1}{k}\) and \(t_{50}=0.693 T_{a v}\) \(\therefore \quad t_{99.9}=10 \times 0.693 T_{a v}=6.93 T_{a v}\)
