10. If a reaction has ΔS = −100 J/K and is spontaneous, what must be true of the surroundings?A) ΔSsurroundings > 100 J/K B) ΔSsurroundings > −100 J/K C) ΔSsurroundings = 100 J/KD) ΔSsurroundings < −100 J/K E) ΔSsurroundings < 100 J/K

Answer : The correct option is, (C) ΔS (surroundings) = 100 J/K

Explanation :

As we know that:

ΔS (total) = ΔS (system) + ΔS (surroundings)

When the reaction is spontaneous ΔS (total) > 0 , that means positive value.

When the reaction is non-spontaneous ΔS (total) < 0 , that means negative value.

As we are given that:

ΔS (system) = -100 J/K       (for spontaneous reaction)

Thus, the ΔS (surroundings) must be greater than ΔS (system) that means positive value.

So, ΔS (surroundings) = 100 J/K

Hence, the correct option is, (C) ΔS (surroundings) = 100 J/K

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.