Following are the values of $E_{a}$ and $ΔH$ for three reactions carried out at the same temperature:
$I:$ $E_{a} = 20 kJ {mol}^{- 1}, Δ H = - 60 kJ {mol}^{- 1}$
$II : E_{a} = 10 kJ {mol}^{- 1}, Δ H = - 20 kJ {mol}^{- 1}$
$III : E_{α} = 40 kJ {mol}^{- 1}, Δ H = + 15 kJ {mol}^{- 1}$
If all the three reactions have same frequency factor then fastest and slowest reactions are :

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$Fastest Slowest$

$I$ $II$

$Fastest Slowest$

$II$ $III$

$Fastest Slowest$

$I$ $II$

can't be predicted

answer is B.

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Detailed Solution

Although the rate of reaction is determined by the value of the rate constant, which depends on activation energy rather than the value of $Δ H$ , it is unquestionably possible to compare the rate of reaction of backward if $Δ H$ values are also provided.

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