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Use the reaction i2(s) i2(g), h = 62.4 kj/mol, s = 0.145 kj/(molk), for question 10. which direction of the reaction is favored at 298 k (room temperature)?

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Let's find the Gibb's free energy for this reaction. The formula is:

G = H- TS
G = (62.4 kJ/mol) - (298 K)(0.145 kJ/mol·K)
G = +19.19 kJ

Now, the sign of G is a criterion for spontaneity. If its sign is -, it means the reaction is spontaneous. Since we got a positive sign, that means the reaction is non-spontaneous. Consequently, the reverse of this reaction would make it negative and spontaneous. Therefore, the favorable reaction is the reverse reaction.

The direction of the reaction is favored at 298 kelvin is in the backward direction as gibbs free energy is positive.

Which factor is used to measure the spontaneity?

The factor which is used to measure the spontaneity or favourable condition of the reaction is gibbs free energy and it will be calculated as:

ΔG = ΔH - TΔS

Given that, chnage in heat or enthalpy = 62.4 kJ/mol

Temperature of the reaction = 298 K

Change in entropy of reaction = 0.145 kJ/mol·K

On putting values on above equation, we get

ΔG = (62.4 kJ/mol) - (298 K)(0.145 kJ/mol·K)

ΔG = 19.19 kJ

From the calculation it is clear that energy is absorbed in the reaction so it will not favor the forward condition, else it favors the bakcward reaction.

Hence reaction is favor in the backward direction.

To know more about spontaneity, visit the below link:

https://brainly.com/question/24279907

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