Question

The activation energy for the reaction no2(g)+co(g)⟶no(g)+co2(g) is ea = 375 kj/mol and the change in enthalpy for the reaction is δh = -225 kj/mol . what is the activation energy for the reverse reaction?

Answer 1

Answer is: 600 kJ/mol.
Chemical reaction: NO₂(g) + CO(g) ⟶ NO(g) + CO₂(g).

Ea(forward) = 375 kJ/mol.
Ea(reverse) = ? kJ/mol.
ΔH(reaction) = -225 kJ/mol; this is exothermic reaction.
The enthalpy change of reaction is the change in the energy of the reactants to the products.
ΔH(reaction) = Ea(forward) - Ea(reverse).
-225 kJ/mol = 375 kJ/mol - Ea(reverse).
Ea(reverse) = 600 kJ/mol.

Answer 2

Activation Energy is the energy that is required to start a reaction. The activation energy for the reverse reaction is 600kJ/ mol.

Activation Energy :

It is the energy that is required to start a reaction. It is denoted by Ea.

The given reaction,

$\bold{NO_2(g)+CO(g)\rightarrow NO(g)+CO_2(g) }$

The enthalpy formula

$\bold {\Delta H(rxn) = Ea(f) - Ea(r).}$

Where,

$\bold {\Delta Hrxn}$ = -225 kj/mol

Ea(f) - Activation energy for farword reaction = 375 kj/mol

Ea(r) - Activation energy for reverse reaction = ?

Put the value in the formula and solve it for Ea(r)

$\bold {-225 kJ/mol = 375 kJ/mol - Ea(reverse).}\\\\\bold {Ea(reverse) = 600 kJ/mol.}$

Therefore, the activation energy for the reverse reaction is 600kJ/ mol.

To know more about activation energy,

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