Consider the following reaction: C2H4(g)+H2(g)→C2H6(g) ΔH=−137.5kJ; ΔS=−120.5J/K Calculate ΔG at 25 ∘C and determine whether the reaction is spontaneous. Express the free energy change in joules to four significant figures.

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sebassandin sebassandin · Answer 1 · 2020-07-13T02:14:04+02:00

Answer:

* [tex]\Delta G=-101.6kJ[/tex]

* Spontaneous reaction.

Explanation:

Hello,

In this case, for the given reaction, we can compute the Gibbs free energy by using the shown below equation:

[tex]\Delta G=\Delta H-T\Delta S[/tex]

In such a way, we proceed as follows with the proper units:

[tex]\Delta G=-137.5kJ-(25+273.15)K*(-120.5\frac{J}{K}*\frac{1kJ}{1000J} )\\\\\Delta G=-101.6kJ[/tex]

Therefore, since the Gibbs free energy of reaction is less than 0, the reaction is said to be spontaneous.

Best regards.

andromache andromache · Answer 2 · 2022-03-24T18:59:17+01:00

The value of ΔG should be -101.6KJ.

The reaction should be Spontaneous.

Here the Gibbs free energy by using the below equation:

So,

=-137.5K - (25 + 273.15)K * (-120.5J/K * 1KH/1000J)

= -101.6KJ

As we can see that the Gibbs free energy of reaction is less than 0, the reaction is said to be spontaneous.

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