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Enthalpy of Combustion

If a reaction...

Question

If a reaction, A + B $\to$ C, is exothermic to the extent of 30 kJ $m o l^{- 1}$ and the forward reaction has an activation energy, $70 k J / m o l^{- 1}$ . The activation energy for the reverse reaction is:

30 kJ

m o l^{- 1}

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40 kJ

m o l^{- 1}

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70 kJ

m o l^{- 1}

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100 kJ

m o l^{- 1}

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Solution

The correct option is A 100 kJ $m o l^{- 1}$
In case of the reverse reaction,
$h e a t + C ⟶ A + B$

The difference between activation energy of the forward reaction and the reverse reaction will be $△ H$ .

$E_{a} r e v e r s e = △ H + E_{a} f o r w a r d$

$\Rightarrow E_{a} r e v e r s e = 30 + 70 k J / m o l$

$= 100 k J / m o l$

Hence, option D is correct.

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If a reaction, A + B → C, is exothermic to the extent of 30 kJ mol−1 and the forward reaction has an activation energy, 70kJ/mol−1. The activation energy for the reverse reaction is:

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