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shutvik [7]
3 years ago
14

If δh°rxn and δs°rxn are both positive values, what drives the spontaneous (favored) reaction and in what direction at standard

conditions?
Chemistry
1 answer:
Arada [10]3 years ago
8 0
In thermodynamics and physical chemistry, the Gibb's free energy is the criterion for spontaneity. If the Gibb's free energy, denoted as ΔG, is negative, then the reaction is spontaneous. If it is positive, it is non-spontaneous. To estimate ΔG, there is a derived relationship between Gibb's free energy, enthalpy and entropy. The equation is

ΔG=ΔH-TΔS, where ΔH and ΔS is the enthalpy and entropy of the reaction, and T is the temperature at which the reaction happens.
So if ΔH and ΔS are both positive, in order to make ΔG negative, T must be very high. In this way, TΔS would be larger than ΔH.

Therefore, a reaction with a positive ΔH and ΔS will be spontaneous at high temperatures.
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3 years ago
In the reaction N2O4(g) 2NO2(g), what changes in color would you expect as pressure is increased at constant temperature?
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Answer:

Brown color of the solution decreases

Explanation:

NO_2 is brown in color whereas N_2O_4 is colorless.

Equilibrium reaction between NO_2 and N_2O_4 is as follows:

2NO_2\leftrightharpoons N_2O_4

As per the Le Chatelier's principle, if pressure of a equilibrium is increased, the equilibrium will shift in the direction having fewer no. of moles of gases.

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