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determine the entropy change for the above reaction from the following standard entropies of the reactants and products:

Sagot :

Qwcold

To determine the entropy changes for a chemical reaction; we have seen that the energy given off (or absorbed) by a reaction, and monitored by noting the change in temperature of the surroundings, can be used to determine the enthalpy of a reaction (example by using a calorimeter).

Changes in internal energy, that are not accompanied by a temperature change, might reflect changes in the entropy of the system. For eg., a change in entropy associated with the Haber process for the production of ammonia from nitrogen and hydrogen gas.

N₂(g) + 3H₂(g) --- 2NH₃(g)

At 298K as a standard temperature:

S°(NH₃) = 192.5 J/molK

S°(H₂) = 130.6 J/molK

S°(N₂) = 191.5 J/molK

Solution,

From the balanced equation we can write the equation for ΔS°(the change in the standard molar entropy for the reaction):

ΔS° = 2*S° (NH₃) - [S°(N₂) + (3*S°(H₂)]

ΔS° = 2* 192.5 - [191.5 + (3*130.6)]

ΔS° = -198.3 J/molK

It would appear that the process results in a decrease in entropy i.e. a decrease in disorder. This is expected because we are decreasing the number of gas molecules.

Learn more about the entropy change here:

https://brainly.com/question/12743264

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