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

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.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

wher is the rest of the question