In the first order reaction 75% of the reactant disappeared in 1.388 hrs. Calculate the rate constant of the reaction :

1 s^{- 1}

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2.8 \times 10^{- 4} s^{- 1}

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17.2 \times 10^{- 3} s^{- 1}

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1.8 \times 10^{- 3} s^{- 1}

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Solution

The correct option is D $2.8 \times 10^{- 4} s^{- 1}$
$k = \frac{2.303}{t} l o g \frac{100}{100 - x}$

$k = \frac{2.303}{1.388 \times 3600} l o g \frac{100}{25}$

$k = 2.8 \times 10^{- 4} s^{- 1}$

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In the first order reaction 75% of the reactant disappeared in 1.388 hrs. Calculate the rate constant of the reaction :

The correct option is D 2.8×10−4s−1k=2.303tlog100100−xk=2.3031.388×3600log10025k=2.8×10−4 s−1

The correct option is D $2.8 \times 10^{- 4} s^{- 1}$
$k = \frac{2.303}{t} l o g \frac{100}{100 - x}$

$k = \frac{2.303}{1.388 \times 3600} l o g \frac{100}{25}$

$k = 2.8 \times 10^{- 4} s^{- 1}$