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Helen [10]
3 years ago
12

An endergonic reaction with a Δh and Δs can be changed into an exergonic reaction.

Chemistry
1 answer:
zheka24 [161]3 years ago
4 0

Full question:

This question is incomplete, here it is completed:

An endergonic reaction with a ______ ∆H and a ______ ∆S can be changed into an exergonic reaction by decreasing the temperature.

Option A: negative, positive

Option B: negative, negative

Option C: positive, positive

Option D: positive, negative

Answer:

Option B: negative, negative

Explanation:

The change in free energy (ΔG) of a system for a constant-temperature process is

ΔG = ΔH - TΔS

free energy is the energy available to do work. Thus, if a particular reaction is accompanied by a release of usable energy (that is, <u>ΔG is negative</u><u>), it is said to be</u><u> exergonic</u>. On the other hand, if a reaction consumes energy (that is, <u>ΔG is positive</u><u>), it is said to be </u><u>endergonic</u>.

Looking at the equation, we can see that if ΔH is negative and ΔS is negative, then ΔG will be negative only when TΔS  is smaller in magnitude than ΔH. This condition is met when T is small.

ΔG = ΔH - TΔS

           -        -

This means that the reaction proceeds spontaneously at low temperatures. At high temperatures, the reverse reaction becomes spontaneous. An example of that would be the following reaction:

NH₃(g) + HCl(g) → NH₄Cl(s)

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what is the pressure, in atmospheres, of 2.97 mol h2 gas if it has a volume of 73 liters when the temperature is 298 k? 0.50 atm
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P x V = n x R x T

P x 73 = 2.97 x 0.082 x 298

P x 73 = 72.57492

P = 72.57492 / 73

P = 1.0 atm

hope this helps!




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