Lattice Energy and Born-Haber Cycles (A Level) Quiz

Derived lesson quiz from the Energetics & Thermodynamics bank focused on lattice-energy trends and Born-Haber-style cycle reasoning.

GCE A-Level H2 Chemistry 9476-2027

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Which statement is Hess’ Law?

Rate depends only on concentration
Enthalpy change is independent of route
Entropy always increases
Catalysts change equilibrium constant

Lattice energy magnitude is generally greater when:

Ions have lower charge and larger radius
Ions have higher charge and smaller radius
Ions have lower charge and smaller radius
Ions have higher charge and larger radius

If a thermochemical equation is reversed, what happens to $\Delta H$?

It stays the same
It changes sign
It becomes zero
It must be multiplied by 2

Use formation enthalpies to find $\Delta H^\ominus$ for $\ce{CH4 + 2O2 -> CO2 + 2H2O(l)}$. Given: $\Delta H_f^\ominus(\ce{CO2})=-394$, $\Delta H_f^\ominus(\ce{H2O(l)})=-286$, $\Delta H_f^\ominus(\ce{CH4})=-75$ kJ mol$^{-1}$.

−891 kJ mol$^{-1}$
−319 kJ mol$^{-1}$
+891 kJ mol$^{-1}$
−75 kJ mol$^{-1}$

Which compound has the most exothermic (most negative) lattice enthalpy of formation?

$\ce{NaCl}$
$\ce{MgO}$
$\ce{KBr}$
$\ce{LiF}$

Lattice enthalpy of formation is the enthalpy change when:

1 mol of ionic solid is separated into gaseous ions
Gaseous ions form 1 mol of ionic solid
1 mol of an ionic solid dissolves in water
1 mol of atoms forms 1 mol of ions in the gas phase

Lattice Energy and Born-Haber Cycles (A Level) Quiz

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