Time required to decompose SO₂ Cl₂ to half its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

Solution

Given that
half life, t_1/2 = 60 min = 60 x 60 = 3600 sec (1 min = 60 sec)
The formula of half life for the a 1^st order

reaction,For a first order reaction.

t = \frac{2.303}{k} \log \frac{1}{a - x} t_{1 / 2} = 60 minutes = 60 \times 60 \sec . = 360 \sec . k = \frac{0.693}{3600 \sec .} = 1.925 \times 10^{- 4} s^{- 1}

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Chemical Kinetics

Time required to decompose SO₂ Cl₂ to half its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

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Time required to decompose SO2 Cl2 to half its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

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What will be the effect of temperature on rate constant?

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Mock Test Series

NCERT Sample Papers

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Time required to decompose SO₂ Cl₂ to half its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

The rate law for the decomposition of N₂O₅ is rate = k[N₂O₅]. What is the significance of k in this equation?