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Ann [662]
3 years ago
8

What describes the change in Gibbs free energy (∆G) of a spontaneous reaction?

Chemistry
1 answer:
alexandr1967 [171]3 years ago
3 0

<u>Answer:</u> The correct answer is Option A.

<u>Explanation:</u>

Gibbs Free energy is defined as amount of useful work that can be done in the system. It is equal to the enthalpy of the reaction minus the product of entropy of the reaction and absolute temperature.

Mathematically,

\Delta G=\Delta H-T\Delta S

Where,

\Delta G = Gibbs free energy

\Delta H = Enthalpy of the reaction

\Delta S = Entropy of the reaction

T = Absolute temperature

Sign Convention for Gibbs Free energy:

If \Delta G, it is considered as a Spontaneous reaction.

If \Delta G>0, it is considered as a Non-Spontaneous reaction.

If \Delta G=0, reaction is in equilibrium.

Hence, the correct answer is Option A.

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Consider the following system at equilibrium:A(aq)+B(aq) &lt;---&gt; 2C(aq)Classify each of the following actions by whether it
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Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

  • On addition of reactant at equilibrium shifts the equilibrium in forward direction.
  • On addition of product at equilibrium shifts the equilibrium in backward direction.
  • On removal of reactant at equilibrium shifts the equilibrium in backward direction.
  • On removal of product at equilibrium shifts the equilibrium in forward direction.

A(aq)+B(aq)\rightleftharpoons 2C(aq)

Reactants = A , B

Product = C

1. Increase A

On increasing the amount of A at equilibrium will shift the equilibrium in forward or rightward direction.

2. Increase B

On increasing the amount of B at equilibrium will shift the equilibrium in forward or rightward direction.

3. Increase C

On increasing the amount of C at equilibrium will shift the equilibrium in backward or leftward direction.

4. Decease A

On decreasing the amount of A at equilibrium will shift the equilibrium in backward or leftward direction.

5. Decease B

On decreasing the amount of B at equilibrium will shift the equilibrium in backward or leftward direction.

6. Decease C

On decreasing the amount of C at equilibrium will shift the equilibrium in forward or rightward direction.

7. Double A and Halve B

Equilibrium constant of the reaction = K

K=\frac{[C]^2}{[A][B]}

On doubling A and halving B, equilibrium constant of the reaction = K'

K'=\frac{[C]^2}{[2A][\frac{B}{2}]}=\frac{[C]^2}{[A][B]}

The value of equilibrium constant K' is equal to K, which means that equilibrium will not shift in any direction.

8. Double both B and C

Equilibrium constant of the reaction = K

K=\frac{[C]^2}{[A][B]}

On doubling B and C, equilibrium constant of the reaction = K'

K'=\frac{[2C]^2}{[A][2B]}=\frac{4[C]^2}{[A][2B]}=\frac{2[C]^2}{[A][B]}

K' = 2 K

The value of equilibrium constant K' is double the K, which means that product is increasing which means that equilibrium will shift in backward or leftward direction.

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3 years ago
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