Energy Changes in Chemical Reactions - SS1 Chemistry Past Questions and Answers - page 4

The reaction occurs rapidly.

The reaction occurs without any external influence.

The reaction occurs with a decrease in entropy.

The reaction occurs at a constant temperature.

 A positive change in Gibbs free energy (ΔG).

A negative change in Gibbs free energy (ΔG).

A zero change in Gibbs free energy (ΔG).

An unpredictable change in Gibbs free energy (ΔG).

ΔG is always positive.

ΔG is always negative.

ΔG can be positive or negative depending on the reaction conditions.

ΔG is always zero.

ΔG = ΔH + ΔS

ΔG = ΔH - ΔS

ΔG = ΔH/ΔS

ΔG = ΔS/ΔH

ΔH > 0 and ΔS > 0

ΔH < 0 and ΔS < 0

ΔH > 0 and ΔS < 0

ΔH < 0 and ΔS > 0

The initial concentrations of reactants.

The activation energy of the reaction.

The sign of ΔG.

Negative

Zero

Cannot be determined

ΔG = 0

ΔG < 0

ΔG > 0

ΔG is not defined for non-spontaneous reactions.

Activation energy with enthalpy change.

Enthalpy changes with entropy change.

Gibbs free energy change with activation energy.

Entropy changes with activation energy.