Melting/Spontaneous Processes


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Tessa Lawler 1A
Posts: 57
Joined: Fri Sep 28, 2018 12:18 am

Melting/Spontaneous Processes

Postby Tessa Lawler 1A » Tue Feb 26, 2019 5:37 pm

In the textbook, it says Because the solid and liquid phases are in equilibrium at the melting point, you should expect to find that
ΔG=0 at 0.°C. Above that temperature the melting of the solid state is favored, so you should expect that ΔG will be negative at 10.°C.
Why does ΔG have to be negative just because the melting of the solid state is favored?

Simmi Diwanji 2B
Posts: 32
Joined: Fri Sep 28, 2018 12:20 am

Re: Melting/Spontaneous Processes

Postby Simmi Diwanji 2B » Wed Feb 27, 2019 1:06 am

When a system is thermodynamically favorable, it means that it has -deltaG because that indicates a spontaneous reaction is occurring. In this case, it is melting.

Lia Inadomi 1I
Posts: 62
Joined: Fri Sep 28, 2018 12:15 am

Re: Melting/Spontaneous Processes

Postby Lia Inadomi 1I » Wed Feb 27, 2019 2:00 pm

A negative delta G value shows that a reaction is spontaneous. The forward reaction in this case is melting so if delta G is negative then that is favored.

daniella_knight1I
Posts: 57
Joined: Fri Sep 28, 2018 12:18 am

Re: Melting/Spontaneous Processes

Postby daniella_knight1I » Wed Feb 27, 2019 3:23 pm

Melting would be a forward reaction so delta G is expected to be negative and favorable because it is spontaneous.


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