Select all of the following statements that are false about ΔGo and ΔG:a) If the reaction has a large negative ΔGo value, the re

Question

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Select all of the following statements that are false about ΔGo and ΔG:a) If the reaction has a large negative ΔGo value, the re

action must reach equilibrium at a small extent of reaction value.b) ΔGo and ΔG can have different values, they don't even have to have the same sign.c) For a reaction that reaches equilibrium, the minimum value of free energy must be at the equilibrium point.d) ΔGo and ΔG have the same magnitude, they just have opposite signs.e) If ΔGo, measured at an extent of reaction = 0.5, is positive, the sign for ΔG when the extent of reaction = 0.80 is also positive.

Chemistry

1 answer:

OLEGan [10] · Answer 1 · 2022-04-19T21:42:49+03:00

Answer:

a) If the reaction has a large negative ΔGo value, the reaction must reach equilibrium at a small extent of reaction value

d) ΔGo and ΔG have the same magnitude, they just have opposite signs.

Explanation:

The fraction of the total heat energy if a system that does useful work is known as Gibb's free energy (G) and the change from the initial to final state is designated by $\Delta G$ . It is observed that the values of $\Delta G$ changes with experimental conditions such as temperature , pressure , concentration etc.

$\Delta G^0$ is the standard free energy change which is a balance of two natural tendencies of any system.

Minimization of potential energy or enthalpic factor $\Delta H^0$

Maximization of disorderliness or entropic factor $T\Delta S^0$

Mathematically; $\Delta G$ = $\Delta H^0$ - $T\Delta S^0$

Thus; from above mentioned, the statements that are true about ΔG⁰ and ΔG are:

ΔG⁰ and ΔG can have different values, they don't even have to have the same sign

For a reaction that reaches equilibrium, the minimum value of free energy must be at the equilibrium point

If ΔG⁰ , measured at an extent of reaction = 0.5, is positive, the sign for ΔG when the extent of reaction = 0.80 is also positive.

while the false statements include:

a) If the reaction has a large negative ΔG⁰ value, the reaction must reach equilibrium at a small extent of reaction value

d) ΔG⁰ and ΔG have the same magnitude, they just have opposite signs.