For a particular reaction, δ h ∘ = 55.4 kj δh∘=55.4 kj and δ s ∘ = 94.1 j/k. δs∘=94.1 j/k. assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous?

The temperature at which the reaction changes from non-spontaneous to spontaneous is 588.735 K

Explanation:

The spontaneity of a reaction is determined by the change in Gibbs Free Energy, .

If is greater than zero, then a reaction is feasible.

If is less than zero, then a reaction is not feasible.

To determine the temperature at which the reaction changes from non-spontaneous to spontaneous, we should equate the to zero.

We take as the limiting condition.

Therefore, the temperature is: 588.735K

particle   p is an electron and particle q is a neutron

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.