If a reaction has a ΔG of -136kJ at 110°C, will it be spontaneous at this temperature (110°C)?

The answer to your question is Yes, it is spontaneous

Explanation:

Gibbs free energy is the sum of the enthalpy plus the product of the temperature and the entropy of the system.

                       G = H - TS

The sign of the Gibbs free energy of a reaction determines if the reaction is spontaneous or nonspontaneous.

If ΔG > 0  the reaction is non-spontaneous

If ΔG < 0 the reaction is spontaneous

In this question ΔG = -136 kJ, then it will be spontaneous.

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

a is the correct answer