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Standard XII

Chemistry

Arrhenius Equation

The activatio...

Question

The activation energy of exothermic reaction, $A ⟶ B$ , is $80$ $k J$ ${m o l}^{- 1}$ . The heat of reaction is $200$ $k J$ ${m o l}^{- 1}$ . The activation energy for the reaction $B ⟶ A$ $(i n k J / m o l)$ will be:

80

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120

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40

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280

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Solution

The correct option is C $280$
$Δ H = E_{f} - E_{b}$
$- 200 = 80 - E_{b}$
$E_{b} = 280 k J / m o l$

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The activation energy of exothermic reaction, A⟶B, is 80 kJ mol−1. The heat of reaction is 200 kJ mol−1. The activation energy for the reaction B⟶A (in kJ/mol) will be:

The correct option is C 280ΔH=Ef−Eb−200=80−EbEb=280kJ/mol

The activation energy of exothermic reaction, $A ⟶ B$ , is $80$ $k J$ ${m o l}^{- 1}$ . The heat of reaction is $200$ $k J$ ${m o l}^{- 1}$ . The activation energy for the reaction $B ⟶ A$ $(i n k J / m o l)$ will be:

The correct option is C $280$
$Δ H = E_{f} - E_{b}$
$- 200 = 80 - E_{b}$
$E_{b} = 280 k J / m o l$