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Chemical Kinetics

Question
CBSEENCH12010702
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For a first order reaction, (A) → products, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is

  • 1.73 x 10–5 M/ min

  • 3.47 x 10–4 M/min

  • 3.47 x 10–5 M/min

  • 1.73 x 10–4 M/min

Solution

B.

3.47 x 10–4 M/min

By first order kinetic rate constant,
straight k space equals space fraction numerator 2.303 over denominator straight t end fraction space log open parentheses fraction numerator straight a over denominator straight a minus straight x end fraction close parentheses straight a space equals space 0.1 space straight M left parenthesis straight a minus straight x right parenthesis space equals space 0.025 space straight M comma space straight t space equals space 40 space min straight k space equals space fraction numerator 2.303 over denominator 40 end fraction space log space fraction numerator 0.1 over denominator 0.025 space straight M end fraction equals space 0.0347 space min to the power of negative 1 end exponent Rate space equals space open parentheses dx over dt close parentheses space equals space straight k left square bracket straight A right square bracket to the power of 1 space equals space 0.0347 space straight x space 0.01 equals space 3.47 space straight x space 10 to the power of negative 4 end exponent space straight M space min to the power of negative 1 end exponent

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?

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction.

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