If it's too much i mainly just need C

Question

 Consider the enthalpy diagram shown below.

a. According to the enthalpy change, would you expect the reaction represented by the diagram to be thermodynamically favorable or unfavorable? Explain. (1 point)

b. Describe a way in which such a reaction might produce large amount of product, despite being thermodynamically unfavorable. (1 point)

c. Consider the reverse reaction, in which the products become the reactants and the reactants become the products. What effect, if any, would this have on the reaction's thermodynamic favorability, the energy of the reaction, and the graph? (2 points)

Answer 1

a. This reaction would be thermodynamically unfavorable. It is unfavorable because the enthalpy of the products in greater than the enthalpy of the reactants. This is actually called an endothermic reaction. It requires an input of energy. A thermodynamically favorable reaction will tend to release energy (exothermic).

b. Increasing the concentration of the reactants, or adding some kind of catalyst will assist in producing more products even in unfavorable conditions.

c. I nearly answered this with my response on A, but not quite. If the reactants and products were switched places, this would be a favorable reaction and would be exothermic (releasing energy). The graph would represent the reactants on the top (higher enthalpy) and the products would have a lower enthalpy on the bottom.

This doesn't cover everything in full, but I hope this leads you in the right direction!