If the first order rate constants for the decomposition of ethyl iodide at 600K and 700K are 2.0×10−5s−1 and 2.0×10−4s−1 respectively, th activation energy for this reaction in kJ mol–1 is

logk2k1=Ea2.303R1T1-1T2log2×10-42×10-5=Ea2.303R1600-1700 Ea=80.4

If the first order rate constants for the decomposition of ethyl iodide at 600K and 700K are 2.0×10−5s−1 and 2.0×10−4s−1 respectively, th activation energy for this reaction in kJ mol–1 is

logk2k1=Ea2.303R1T1-1T2log2×10-42×10-5=Ea2.303R1600-1700 Ea=80.4

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If the first order rate constants for the decomposition of ethyl iodide at 600K and 700K are $2.0 \times 10^{- 5} s^{- 1} and 2.0 \times 10^{- 4} s^{- 1}$ respectively, th activation energy for this reaction in kJ mol^–1 is

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60.3

40.2

80.4

20.1

answer is A.

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$\log \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

$\log \frac{2 \times 10^{- 4}}{2 \times 10^{- 5}} = \frac{E_{a}}{2.303 R} [\frac{1}{600} - \frac{1}{700}] E_{a} = 80.4$

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If the first order rate constants for the decomposition of ethyl iodide at 600K and 700K are 2.0×10−5s−1 and 2.0×10−4s−1 respectively, th activation energy for this reaction in kJ mol–1 is

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If the first order rate constants for the decomposition of ethyl iodide at 600K and 700K are $2.0 \times 10^{- 5} s^{- 1} and 2.0 \times 10^{- 4} s^{- 1}$ respectively, th activation energy for this reaction in kJ mol^–1 is