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GRE Subject Test: Chemistry : Endergonic and Exergonic Reactions

Study concepts, example questions & explanations for GRE Subject Test: Chemistry

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Example Questions

Example Question #1 : Endergonic And Exergonic Reactions

The equation for the change in Gibbs free energy is given below.

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

ΔH = change in enthalpy

ΔS = change in entropy

Which of the following scenarios guarantees a nonspontaneous reaction?

Possible Answers:

When ΔH is negative and ΔS is negative

When ΔH is positive and ΔS is negative

When ΔH is negative and ΔS is positive

When ΔH is positive and ΔS is positive

Correct answer:

When ΔH is positive and ΔS is negative

Explanation:

A positive value for ΔG (Gibbs free energy) will guarantee a nonspontaneous reaction. When ΔH (enthalpy) is postive and ΔS (entropy) is negative, the change in Gibbs free energy must be positive and, therefore, nonspontaneous.

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

$\Delta G=(+)-T(-)=(+)+(+)=+$

Because T (temperature) will always have a positive value, a negative entropy and positive enthalpy will always result in a positive Gibbs free energy.

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Example Question #1 : Endergonic And Exergonic Reactions

The equation for the change in Gibbs free energy is given below.

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

ΔH = change in enthalpy

ΔS = change in entropy

In which of the scenarios will the reaction be spontaneous?

Possible Answers:

When both ΔH and ΔS are postive and T is high

When ΔH is negative and ΔS is postive

When both ΔH and ΔS are negative and T is low

All of these scenarios would result in spontaneous reactions

Correct answer:

All of these scenarios would result in spontaneous reactions

Explanation:

All of the following scenarios would lead to spontaneous reaction, since each scenario would result in a negative Gibbs free energy (-ΔG).

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

Negative enthalpy, positive entropy:

$\Delta G=(-)-T(+)=(-)+(-)=-$

Positive enthalpy and entropy with high temperature:

$\Delta G=(+)-(+++)(+)=(+)+(---)=-$

Negative enthalpy and entropy with low temperature:

$\Delta G=(-)-(+)(-)=(-)+(-)=-$

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Example Question #81 : Physical Chemistry

Which of the following scenarios describes a reaction in equilibrium?

Possible Answers:

When $\DeltaH$ $\Delta H$ is equal to $T\Delta S.$

When Gibbs free energy is negative

When the forward rate is 0M/s

When the enthalpy is equal to the entropy

Correct answer:

When $\DeltaH$ $\Delta H$ is equal to $T\Delta S.$

Explanation:

According to the Gibbs free energy equation, a system is at equilibrium when $\Delta G$ is equal to 0.

Since $\Delta G = \Delta H - T\Delta S$ , a system is in equilibrium when $\Delta H = T\Delta S$ . A negative Gibbs free energy means that the reaction will be spontaneous. At equilibrium, the forward reaction rate equals the reverse reaction rate, though the net rate is zero.

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GRE Subject Test: Chemistry : Endergonic and Exergonic Reactions

Study concepts, example questions & explanations for GRE Subject Test: Chemistry

All GRE Subject Test: Chemistry Resources

Example Questions

Example Question #1 : Endergonic And Exergonic Reactions

Example Question #1 : Endergonic And Exergonic Reactions

Example Question #81 : Physical Chemistry

All GRE Subject Test: Chemistry Resources

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