Spontaneous
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Spontaneous
Can someone clarify how to prove when a reaction is spontaneous using Gibbs Free Energy?
Re: Spontaneous
A reaction is spontaneous where deltaG is negative. When deltaG is positive the reaction is non spontaneous.
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Re: Spontaneous
A reaction is spontaneous when delta G is negative. for this to happen either delta H has to be negative, delta S has to be positive, or both are true. these factors creative spontaneity by driving the reaction either by enthalpy or entropy.
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Re: Spontaneous
If you use the G = H - TS, with a - H and + s, you will have a spontaneous reaction. If you have a +H and -S, the reaction will be non-spontaneous. If both are positive, the reaction will be spontaneous if TS is greater than H. If both are negative, the reaction will be spontaneous if H is greater than TS.
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Re: Spontaneous
When Delta G is negative, the reaction is exothermic. This means that it releases heat and does not require an input of energy; hence, it is spontaneous. An exothermic reaction indicates that an input of energy is required. This makes it a non-spontaneous reaction as it needs something else (not spontaneous) to make it do work.
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Re: Spontaneous
If delta G is negative then it is spontaneous, and if it is positive then it is not spontaneous.
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Re: Spontaneous
If gibbs free energy is less than zero, it is spontaneous. There is a chart in the book to correlate the two parts of gibbs free, the enthalpy and entropy part of the equation.
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Re: Spontaneous
If delta G (the measure of Gibb's free energy) is positive, the reaction is not spontaneous. If it is negative, the reaction is spontaneous and therefore favorable.
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