The following reation has the following standard thermodynamic parameters: change in H= -35.1 kJ/mol and change in S= -67.3 J/(mol x K). C(g) + D(g) --> E(g)

Is the reaction exothermic or endothermic?

Does the negative entropy change make sense?
A. No, because the number of independently moving particles decreases.
B. Yes, because the number of independently moving paticles increases.
C. No, because the number of independently moving particles increases.
D. Yes, because the number of independently moving particles decreases.

Is the reation spontaneous at all temperatures? If not, explain.

A. The reaction will be spontaneous at high temperatures because increasing the temperature of a system with a negative change in S eventually results in a positive change in G.

B. The reaction will be spontaneous at low temperatures because increasing the temperature of a system with a negative change in S eventually results in a positive change in G.

C. The reaction will be spontaneous at all temperatures.

Calculate the temperature at which the reaction becomes nonspontaneous?