Melting of ice

[Jose Torres]

Would the melting of ice on a hot summer day correlate with or ?

[WilliamNguyen_4L]

Delta G is less than 0.

[Sheridan Slaterbeck 1J]

a solid to a liquid would be a spontaneous reaction so delta G would be negative.

[MichaelMoreno2G]

As mentioned above, Delta G would be less than zero because the reaction is spontaneous.

[Michelle Nwufo 2G]

As mentioned above, Delta G would be less than zero because the reaction is spontaneous.

But how do you determine whether the reaction is spontaneous or not?

[Jonny Schindler 1A]

if you can assume the sign of the enthalpy and entropy you can sometimes use that to determine the sign of delta G.

[Angel Chen 2k]

You can determine if a reaction is spontaneous by examining mainly two factors, the entropy and whether the reaction is exothermic or endothermic. Then by plugging in these values into the Gibss free energy equation, if the answer is negative, then the reaction is spontaneous.

[Hannah Yates 1K]

The melting of ice on a hot summers day would be spontaneous, so delta g would be negative

[Maddy Mackenzie]

The way I looked at this question was to say that if ice was melting, delta H was positive because you are putting heat into the system. Then you can say that delta s is positive because the molecules are going to have more possible positions in a liquid than in a solid. Then if the snow is melting, the temperature must be high enough for the entropy to overcome the enthalpy and cause the delta G to be negative.

[Alysa Rallistan 2G]

This is a spontaneous reaction (dG <0 ) you can look at it as there is no work being done to the system to cause the ice to melt other than an exchange of heat from the sun to the solid ice