For the conversion of ice to water at 0°c and 1 atm,1.δg is negative,δh is negative, and δs is positive.2.δg is zero, δh is positive, and δs is positive.3.δg is positive, δh is negative, and δs is positive.4.δg is zero, δh is positive, and δs is negative.

2. ΔG is zero, ΔH is positive, and ΔS is positive

Explanation:

When the ice is being converted to water ate 0ºC and 1 atm, there is an equilibrium between the solid and the liquid. At the equilibrium point, ΔG (the free energy) is zero. It is negative for spontaneous reactions and positive for nonspontaneous reactions.

For the phase change happens, the ice must absorb heat from the surroundings, so it's an endothermic reaction, and because of that ΔH (the enthalpy) must be positive. It is negative for exothermic reactions.

In the liquid state, the molecules have more energy and the randomness is higher than the solid-state. The entropy (S) is the measure of the randomness, so if it's increasing, ΔS must be positive.

it is b that is the answer.