Question

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The thermal decomposition of HCO2H is a first order reaction with a rate constant of 2.4 × 10-3 s-1 at a certain temperature. Calculate how long will it take for three-fourths of initial quantity of HCO2 H to decompose. (log 0.25 = -0.6021)
(All India 2011)

Answer 1

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Answer 2

→ Given Question:-

→ The thermal decomposition of HCO2H is a first-order reaction with a rate constant of 2.4 × 10-3 s-1 at a certain temperature. Calculate how long will it take for three-fourths of the initial quantity of HCO2 H to decompose. (log 0.25 = -0.6021)

(All India 2011)

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→ Given in the Question:-

⇒  K =  2.4 × 10^-3 3^-1

⇒ According to the given question,

⇒  K  = $\frac{2.303}{t}$ $log$ $\frac{[HCOOH] 0}{[HCOOH]t}$

⇒ [HCOOH]t = [HCOOH]0 - $\frac{3}{4}$ [HCOOH]0 =

⇒ $\frac{1}{4}$ [HCOOH]0

⇒ Now , we have to substitute for [HCOOH],

⇒ K = $\frac{2.303}{t}$ $log$ $\frac{[HCOOH]0}{\frac{1}{4} [HCOOH]0}$

⇒ K =  $\frac{2.303}{t}$$[ log 1 - log 0.25 ]$

⇒ K = $\frac{2.303}{t}$ $[log 1 - log 0.25 ]$

⇒ $t = \frac{2.303 X 0.6021s}{2.4 X 10^-3} =$

⇒ $5.78 X 10^2s$ is your answer.

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