Exam code: YCH11
The enthalpy change of solution of sodium sulfate, Na2SO4 , may be calculated using three pieces of data.
Which of these pieces of data is not required?
lattice energy of Na2SO4
enthalpy change of hydration of Na+
enthalpy change of formation of Na2SO4
enthalpy change of hydration of
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A simplified Born-Haber cycle for the formation of lithium iodide is shown.
The enthalpy change of atomisation of iodine (+107 kJ mol–1) is given by the equation
1⁄2I2(g) → I(g)
1⁄2I2(s) → I(g)
I2(g) → 2I(g)
I2(s) → 2I(g)
Use the information in the cycle to calculate the electron affinity of iodine.
–298 kJ mol–1
–242 kJ mol–1
+242 kJ mol–1
+298 kJ mol–1
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This question is about four ionic compounds.
Which of these compounds would be expected to have the least exothermic lattice energy?
calcium chloride
magnesium chloride
potassium bromide
sodium bromide
Which of these compounds would be expected to have the largest difference between their experimental (Born–Haber) and theoretical lattice energies?
calcium chloride
magnesium chloride
potassium bromide
sodium bromide
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The diagram shows the Born-Haber cycle for magnesium chloride.
Which of these is the electron affinity of chlorine?
y
y/2
(w + y)
(w + y)/2
Which expression gives the lattice energy (LE) for magnesium chloride?
LE = u − (v + w + x + y)
LE = v + w + x + y − u
LE = y − u − (v + w + x)
LE = v + w + x − y + u
Which energy change in the cycle does x represent?
the first ionisation energy of magnesium
the second ionisation energy of magnesium
the sum of the first and second ionisation energies of magnesium
the sum of the enthalpy change of atomisation and the first and second ionisation energies of magnesium
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Aqueous ammonia is titrated with hydrochloric acid.
Which of these is the most suitable indicator for this titration?
Indicator | pH range | |
|---|---|---|
A | Bromothymol blue | 6.0–7.6 |
B | Methyl orange | 3.1–4.4 |
C | Phenol red | 6.8–8.4 |
D | Phenolphthalein | 8.3–10.0 |
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Some energy changes are given in the table.
Energy change | Value / kJ mol–1 |
Lattice energy for CaCl2(s) | –2258 |
Enthalpy change of solution of CaCl2(s) | –120 |
Enthalpy change of hydration of Cl–(g) | –364 |
Use these data to calculate the enthalpy change of hydration of Ca2+(g).
–1410 kJ mol–1
–1650 kJ mol–1
–2014 kJ mol–1
–3106 kJ mol–1
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