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A reaction has an enthalpy change of [tex]-54 \, \text{kJ}[/tex] and an activation energy of [tex]89 \, \text{kJ}[/tex]. What is the enthalpy change of the reverse reaction?

A. [tex]-54 \, \text{kJ}[/tex]
B. [tex]54 \, \text{kJ}[/tex]
C. [tex]-89 \, \text{kJ}[/tex]
D. [tex]89 \, \text{kJ}[/tex]

Answer :

In this case, the forward reaction has an enthalpy change of -54 kJ. Option A

The enthalpy change of the reverse reaction can be determined by applying Hess's law, which states that the enthalpy change of a reverse reaction is equal in magnitude but opposite in sign to the forward reaction. In this case, the forward reaction has an enthalpy change of -54 kJ.

Therefore, the enthalpy change of the reverse reaction is +54 kJ (positive because it is the opposite sign of the forward reaction). This means that the reverse reaction is endothermic, absorbing energy from the surroundings rather than releasing it.

So, the correct answer is B. 54 kJ. The enthalpy change of the reverse reaction is positive 54 kJ. It is important to note that activation energy does not affect the enthalpy change of a reaction. Activation energy is the energy barrier that must be overcome for a reaction to occur, but it does not determine the magnitude or sign of the enthalpy change. Option A is correct.

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