For the reaction2Na(s)+ 2H2O(l)2NaOH(aq) + H2(g)H° = -369 kJ and S° = -15.3 J/KG° would be less than zero at temperatures (above, below)     _____   Enter above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.

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Asked Jul 31, 2019
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  1. For the reaction

    2Na(s)2H2O(l)2NaOH(aq) + H2(g)

    H° = -369 kJ and S° = -15.3 J/K

    G° would be less than zero at temperatures (above, below)     _____   

    Enter above or below in the first box and enter the temperature in the second box. Assume that H° and S° are constant.
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Expert Answer

Step 1

When the value of G° is less than zero, that is G° is negative, the reaction would be spontaneous at all temperatures.  If G° is positive, then the reaction would be non-spontaneous at all temperatures.

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AG AH TAS

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Step 2

When ΔH and ΔS both are either positive or negative, we can determine the temperature at which a nonspontaneous reaction becomes spontaneous or a spontaneous reaction becomes nonspontaneous, because it is the temperature at which the reaction is at equilibrium. 

At equilibrium,

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AG AH TAS = 0

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Step 3

So, the crossover temperature at which a reaction changes ...

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AH T AS

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