Entropy and Gibbs Free Energy (A Level) Quiz

Derived lesson quiz from the Energetics & Thermodynamics bank focused on entropy trends, ΔG calculations, and feasibility conditions.

GCE A-Level H2 Chemistry 9476-2027

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An exothermic reaction has:

$\Delta H > 0$
$\Delta H < 0$
$E_a < 0$
$\Delta S < 0$ always

A reaction is feasible under standard conditions when:

$\Delta G^\ominus > 0$
$\Delta G^\ominus < 0$
$\Delta H^\ominus < 0$ only
$\Delta S^\ominus < 0$ only

A reaction mixture in a thermally insulated container warms without external heating. The reaction is:

endothermic
exothermic
at equilibrium
irreversible

For the Haber process reaction $\ce{N2(g) + 3H2(g) -> 2NH3(g)}$, the sign of $\Delta S$ is most likely:

positive
negative
zero
cannot be predicted

Which option gives $\Delta G$ at 298 K for a reaction with $\Delta H=+50.0$ kJ mol$^{-1}$ and $\Delta S=+200$ J mol$^{-1}$ K$^{-1}$?

−9.6 kJ mol$^{-1}$
+9.6 kJ mol$^{-1}$
−59.6 kJ mol$^{-1}$
+59.6 kJ mol$^{-1}$

For a reaction with $\Delta H>0$ and $\Delta S>0$, the reaction is more likely to be feasible when:

temperature is high
temperature is low
pressure is high
a catalyst is added

Entropy and Gibbs Free Energy (A Level) Quiz

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