Question

1. Which of the following statements are true? Choose all that apply.
   1. ΔGo is temperature independent
   2. Knowing the sign of ΔS_univallows you to determine if a reaction is spontaneous or not
   3. If ΔH^o is negative the reaction will be spontaneous
   4. ΔSorxn and ΔSosur will always have the opposite sign
   5. ΔHo is the energy free to do work in a reaction

Answer 1

In this question,1,2 and 4 are correct.

ΔGo is temperature independent (true)because it is measured at standard conditions, that is at 298-degree Celcius.so for a particular reaction it will be a constant and will not change with respect to the temperature.

according to the second law of thermodynamics, all changes that are spontaneous will lead to an increase in the entropy of the universe.and all changes that are not spontaneous will lead to a decrease in the entropy of the universe. therefore the second statement is true

this statement is not always true. if entropy is positive, we can say that the reaction is spontaneous.therefore (ΔH-ΔG)/T which is equal to ΔS should be positive.here in the question, it is mentioned ΔH^o is negative.then in this condition,ΔG⁰ should be negative or its value sholud be less than ΔH^o for entropy to be positive(to become spontaneous)

The signs of the system and surroundings are opposite to one another because in this case when one releases heat,the other absorbs and vice versa.

standard enthalpy(ΔHo) is the sum of internal energy and pressure volume energy.while energy free to do work in a reaction is given by the gibbs free energy.