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For a reaction the activation energy is zero. What is the value of rate constant at $300 K$ .
[Given $k_{280 K} = 1.6 \times 10^{6} s^{- 1}; R = 8.314 {Jmol}^{- 1} K^{- 1}$ ]

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2.08 \times 10^{- 3}

2.08 \times 10^{- 2}

1.6 \times 10^{6}

6.93 \times 10^{- 2}

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detailed solution

Correct option is C

Given $T_{1} = 280 K, k_{1} = 1.6 \times 10^{6} s^{- 1}, k_{2} = ?, E_{a} = 0, T_{2} = 300 K$ .
By Arrhenius equation,

$\log \frac{k_{1}}{k_{1}} = \frac{E_{a}}{2.303 R} [\frac{T_{2} - T_{1}}{T_{2} T_{1}}] As, E_{a} = 0 or \frac{k_{2}}{k_{1}} = 1 or k_{2} = k_{1} Thus, the rate constant at 300 K is 1 .6 \times 10^{6} s^{- 1}$

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2023 | www.infinitylearn.com

For a reaction the activation energy is zero. What is the value of rate constant at 300 K.[Given k280 K=1.6×106 s-1;R=8.314Jmol-1 K-1 ]

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For a reaction the activation energy is zero. What is the value of rate constant at $300 K$ .
[Given $k_{280 K} = 1.6 \times 10^{6} s^{- 1}; R = 8.314 {Jmol}^{- 1} K^{- 1}$ ]