For a reaction, the energy of activation is zero. The value of rate constant at 300 K, if k = $1.6 \times 10^{6} s^{- 1}$ at 280 K is:

1.60 \times 10^{6} s^{- 1}

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1.56 \times 10^{6} s^{- 1}

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1.82 \times 10^{6} s^{- 1}

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Solution

The correct option is A $1.60 \times 10^{6} s^{- 1}$
$E_{a} = 0$
$∴ l o g \frac{k_{2}}{k_{1}} = 1$
or $k_{2} = k_{1} = 1.6 \times 10^{6} s^{- 1}$

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(IIT-JEE, 2009)

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For a reaction, the energy of activation is zero. The value of rate constant at 300 K, if k = 1.6×106s−1 at 280 K is:

The correct option is A 1.60×106s−1Ea=0∴logk2k1=1or k2=k1=1.6×106s−1

For a reaction, the energy of activation is zero. The value of rate constant at 300 K, if k = $1.6 \times 10^{6} s^{- 1}$ at 280 K is:

The correct option is A $1.60 \times 10^{6} s^{- 1}$
$E_{a} = 0$
$∴ l o g \frac{k_{2}}{k_{1}} = 1$
or $k_{2} = k_{1} = 1.6 \times 10^{6} s^{- 1}$