# Question a5da3

Jun 16, 2015

The energy of the reactant(s) is $\text{+233 kJ}$.

#### Explanation:

The information given to you describes an exothermic reaction because the activation energy of the reverse reaction is smaller than the activation energy of the forward reaction.

This implies that the products are lower in energy than the reactants. As a result, you should expect the energy of the reactants to exceed the energy of the products.

A generic potential energy diagram for an exothermic reaction looks like this

I won't go into the details about what activation energy and threshold energy are, but you can read more on that here:

http://socratic.org/questions/what-is-activation-energy-what-is-threshold-energy-i-want-to-know-the-difference?source=search

So, in your case, the forward reaction has an activation energy equal to

${E}_{\text{a for" = "+96 kJ}}$

The reverse reaction has an activation energy equal to

${E}_{\text{a rev" = "+295 kJ}}$

Moreover, you know that the nergy level of the products is equal to

${E}_{\text{p" = "+34 kJ}}$

This means that the threshold energy of the reaction, i.e. the average kinetic energy that molecules need to react, can be determined by adding the activation energy of the reverse reaction to the energy of the products.

${E}_{\text{TS" = E_"a rev" + E_"p}}$

${E}_{\text{TS" = 295 + 34 = "+329 kJ}}$

So, in order to get a reaction, your molecules need to have an average kinetic energy of +329 kJ. Since you know what the activation energy of the forward reaction is, you can determine the energy of the reactants by

${E}_{\text{TS" = E_"a for" + E_"r}}$

E_"r" = E_"TS" - E_"a for" = 329 - 96 = color(green)("+233 kJ")#

The enthalpy change of reaction will be negative, since the energy of the products is lower than the energy of the reactants.

$\Delta {H}_{\text{rxn" = H_"products" - H_"reactants}}$

$\Delta {H}_{\text{rxn" = 34 - 233 = "-199 kJ}}$

The minus sign symbolizes the fact that heat is released by the reaction.