Which of the following statements is false?

Question

Heat can be considered a "product" in exothermic reactions.
If a reaction is endothermic and has a negative entropy change, we can assume that it is nonspontaneous.
If a reaction is exothermic and has a positive entropy change, we can assume that it is spontaneous.
If two moles of gas react to form one mole of liquid, we can assume that the reaction is spontaneous.

Answer 1

The false answer is
If two moles of gas react to form one mole of liquid, we can assume that the reaction is spontaneous.

Spontaneity can only be determined thermodynamically. Just because two moles of gas have reacted doesn't tell us anything about what was chemically/energetically required to make them react.

Answer 2

the third statement is false, you have to know the enthalpy change - a reaction with a negative entropy change can be spontaneous if the enthalpy term (delta H) is negative and the absolute value of it is larger than the T(delta S) term - but it will be always be nonspontaneous if positive

Answer 3

First statement is true, as the energy of the reactants is higher than that of the products.
Second statement is true, as delta G = delta H - T delta S, and a positive delta H and a negative delta S will give a positive delta G.
Third is also true, but for the opposite reason as #2. Negative delta H and positive delta S will give a negative delta G.
Fourth is false. It may be spontaneous, but it doesn't have to be.

Answer 4

The last one.

Answer 5

I don't know about the moles, but my yard dose have Gophers.AND judging by all the mounds, I would say they react to each other quite often.........