For a reaction, activation energy E_a = 0 and the rate constant at 200 K is 1.6 × 10^6 s^-1 . The rate constant at 400 K will be: - CHEMISTRY MCQ NEET 2019 2026 | ExamTest.live

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For a reaction, activation energy E_{a} = 0 and the rate constant at 200 K is 1.6 \times 1 0^{6} s^{- 1} . The rate constant at 400 K will be:

Solution & Step-by-step Explanation

According to the Arrhenius equation: lo g \frac{k _{2}}{k _{1}} = \frac{E _{a}}{2.303 R} (\frac{T _{2} - T _{1}}{T _{1} T _{2}}) Since E_{a} = 0, the entire right side of the equation becomes zero. lo g \frac{k _{2}}{k _{1}} = 0 ⟹ \frac{k _{2}}{k _{1}} = 1 0^{0} = 1 ⟹ k_{2} = k_{1} .Thus, the rate constant remains 1.6 \times 1 0^{6} s^{- 1} regardless of the temperature change.

Try it yourself before checking the explanation above.

For a reaction, activation energy E_{a} = 0 and the rate constant at 200 K is 1.6 \times 1 0^{6} s^{- 1} . The rate constant at 400 K will be:

3.2 \times 1 0^{4} s^{- 1}

1.6 \times 1 0^{6} s^{- 1}

1.6 \times 1 0^{3} s^{- 1}

3.2 \times 1 0^{6} s^{- 1}

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