## Melting of ice

$\Delta G^{\circ} = -nFE_{cell}^{\circ}$

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Jose Torres
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### Melting of ice

Would the melting of ice on a hot summer day correlate with $\Delta G<0$ or $\Delta G>0$?

WilliamNguyen_4L
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### Re: Melting of ice

Delta G is less than 0.

Sheridan Slaterbeck 1J
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### Re: Melting of ice

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

MichaelMoreno2G
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### Re: Melting of ice

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

Michelle Nwufo 2G
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### Re: Melting of ice

MichaelMoreno2G wrote: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
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### Re: Melting of ice

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
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### Re: Melting of ice

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
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### Re: Melting of ice

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

Maddy Mackenzie
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### Re: Melting of ice

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
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### Re: Melting of ice

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

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