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Chemical Kinetics

Question

75% of a reaction of the first order was completed in 32 minutes. When was its half-life completed?

Solution

The first order reaction can be
$t = \frac{2.303}{k} \log \frac{a}{a - x} w e h a v e g i v e n t = 32 l e t a = 100 x = 75 t h u s p u t t i n g t h e v a l u e i n a b o v e e q u a t i o n 32 = \frac{2.303}{k} l o g \frac{100}{100 - 75} 32 = \frac{2.303}{k} l o g \frac{100}{25} 32 = \frac{2.303}{k} l o g 4 k = \frac{2.303}{32} l o g 4 k = 0.07196 \log 4 k = 0.07196 x 0.6020 k = 0.0433 h a l f - t i m e r e a c t i o n o f f i r s t o r d e r c a n b e g i v e n b y t_{1 / 2} = \frac{0.693}{k} t_{1 / 2} = \frac{0.693}{0.0433} = 16$

Ans. 16 minutes

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

75% of a reaction of the first order was completed in 32 minutes. When was its half-life completed?

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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