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PLEASE HELP> WILL GIVE BRAINLIEST

1. What is Gibbs free energy?
a. The energy contained within the bonds of molecules
b. The usable energy released or absorbed by a reaction
c. The energy in the form of kinetic energy in a system
d. The energy lost as heat to the surrounding molecules

2. What is ΔH in the equation ΔG = ΔH - TΔS?
a. The change in specific heat between the products and the reactants
b. The change in free energy between the products and the reactants
c. The change in entropy between products and reactants in a reaction
d. The change in enthalpy between products and reactants in a reaction

3. What would cause entropy to increase in a reaction?
a. The products becoming more spread out
b. The products forming fewer molecules
c. The products forming a more rigid structure
d. The products forming an ordered pattern

4. What information does Gibbs free energy give about a reaction?
a. It tells what the most stable forms of the products are.
b. It tells if the reaction will proceed spontaneously or not.
c. It tells how quickly the reaction will proceed to equilibrium.
d. It tells what the activation energy of the forward reaction is.

5. For which of the reactions listed below will Gibbs free energy always be negative?
a. An endothermic reaction that increases in entropy
b. An exothermic reaction that decreases in entropy
c. An endothermic reaction that decreases in entropy
d. An exothermic reaction that increases in entropy

Respuesta :

Here is the answer to your first question: In thermodynamics, the Gibbs free energy is a thermodynamic potential that can be used to calculate the maximum of reversible work that may be performed by a thermodynamic system at a constant temperature and pressure. The Gibbs free energy (
Δ
G
=
Δ
H
−
T
Δ
S
{\displaystyle \Delta G=\Delta H-T\Delta S}, measured in joules in SI) is the maximum amount of non-expansion work that can be extracted from a thermodynamically closed system (can exchange heat and work with its surroundings, but not matter). This maximum can be attained only in a completely reversible process. When a system transforms reversibly from an initial state to a final state, the decrease in Gibbs free energy equals the work done by the system to its surroundings, minus the work of the pressure forces.[1]

Answer:

1. b. The usable energy released or absorbed by a reaction

2. d. The change in enthalpy between products and reactants in a reaction

3. a. The products becoming more spread out

4. b. It tells if the reaction will proceed spontaneously or not.

5. d. An exothermic reaction that increases in entropy

Explanation:

1. The definition is the answer (you should try to memorize it)

2. ΔH is change in enthalpy (ΔS is change in entropy)

3. Entropy is the measure of randomess. The more spread out the products are, the higher the entropy.

4. If ΔG was positive, it would be nonspontaneous, if ΔG was negative, it's spontaneous.

5. ΔH is change in enthalpy, and exothermic is releasing heat so ΔH is nugative. ΔS is change in entropy and if entropy is increasing, ΔS is positive. Thus, ΔG  is always negative in this case.

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