Ncert Exercises & Solutions

Consider a certain reaction A → Products with k = 2.0 × 10^–2s^–1. Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L^–1.

k = 2 . 010^{- 2} s^{- 1} T = 100 s

{[A]}_{0} = 1.0 m o l^{- 1}

Since the unit of k is s

^{- 1}

, the given reaction is a first order reaction.

k = \frac{2.303}{t} \log \frac{{[A]}_{0}}{[A]}

Therefore,

\Rightarrow 2.0 \times 10^{- 2} s^{- 1} = \frac{2.303}{100 s} \log \frac{[1.0]}{[A]}

\mapsto 2.0 \times 10^{- 2} s = \frac{2.303}{100 s} (- \log [A])

\Rightarrow - \log [A] = \frac{2.0 \times 10^{- 2} \times 100}{2.303}

\Rightarrow [A] = a n t i \log (- \frac{2.0 \times 10^{- 2} \times 100}{2.303})

= 0.135 mol L

^{- 1}

(approximately)

Hence, the remaining concentration of A is 0.135 mol L

^{- 1}

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