Which of the following represents the second ionisation energy of strontium?
Sr+ (s) → Sr2+ (aq) + e-
Sr (s) → Sr2+ (g) + 2e-
Sr+ (g) → Sr2+ (g) + e-
Sr (g) → Sr2+ (g) + 2e-
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Which of the following represents the second ionisation energy of strontium?
Sr+ (s) → Sr2+ (aq) + e-
Sr (s) → Sr2+ (g) + 2e-
Sr+ (g) → Sr2+ (g) + e-
Sr (g) → Sr2+ (g) + 2e-
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Ammonia is produced according to the following gas-phase synthesis:
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Thermodynamic data for the components of this equilibrium are:
Substance |
N2 (g) |
H2 (g) |
NH3 (g) |
SӨ (J K-1 mol-1) |
191.5 |
130.6 |
192.5 |
The standard entropy change for this reaction is
-129.6 J K-1 mol-1
-198.3 J K-1 mol-1
198.3 J K-1 mol-1
514.6 J K-1 mol-1
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Which of the following is the correct equation for Gibbs free energy?
ΔG = ΔH - TΔS
ΔG = ΔH + TΔS
ΔG = TΔS - ΔH
ΔG = ΔS + TΔH
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The reaction between graphite and oxygen is as follows
C (s) + O2 (g) → CO2 (g) ΔHꝋf = -394 kJ mol-1
The entropy change for this reaction is (+)3 J K-1 mol-1. The free energy change for this reaction at 298 K is
-395 kJ mol-1
-1288 kJ mol-1
-500 kJ mol-1
393 kJ mol-1
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Which of the following best explains why lithium oxide has a much larger lattice enthalpy than potassium oxide?
Lithium ions have a greater charge than potassium ions
Potassium oxide has a greater Mr than lithium oxide
Potassium ions have a greater charge than lithium ions
Lithium ions have a smaller ionic radius than potassium ions
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Which of the following represents the first electron affinity of oxygen?
O (g) + e- → O- (g)
2O (g) + 2e- → 2O- (g)
O (g) + 2e- → O2- (g)
O- (g) → O (g) + e-
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Ethene is produced according to the following gas-phase synthesis:
2C (s) + 2H2 (g) → C2H4 (g)
Thermodynamic data for the components of this equilibrium are
Substance |
C (s) |
H2 (g) |
C2H4 (g) |
ΔHϴf (kJ mol-1) |
0 |
0 |
52 |
Sϴ (J K-1 mol-1) |
6 |
131 |
219 |
The free energy change for this reaction at 330 K is:
+ 18202 kJ mol-1
+ 33.83 kJ mol-1
+ 70.15 kJ mol-1
-18098 kJ mol-1
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Which of the following conditions will mean a reaction is never feasible?
ΔH |
ΔS |
Temperature |
|
A |
Negative |
Positive |
High |
B |
Positive |
Negative |
High |
C |
Negative |
Negative |
Low |
D |
Positive |
Positive |
High |
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Which of the following will show the least covalent character?
Beryllium bromide
Aluminium bromide
Potassium bromide
Magnesium bromide
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Thermodynamic data for the components for magnesium oxide are
Name of enthalpy change |
Energy change (kJ mol-1) |
Enthalpy of formation of magnesium oxide |
-602 |
Enthalpy of atomisation of magnesium |
+150 |
First ionisation energy of magnesium |
+738 |
Second ionisation energy of magnesium |
+1450 |
Enthalpy of atomisation of oxygen |
+248 |
First electron affinity of oxygen |
-142 |
Second electron affinity of oxygen |
+844 |
The lattice enthalpy of formation for magnesium oxide is:
-4174 kJ mol-1
-3890 kJ mol-1
-3766 kJ mol-1
-4138 kJ mol-1
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Using the information in the table to answer the question
Ion |
Value (kJ mol-1) |
ΔHӨlatt CaF2 |
(+)2651 |
ΔHӨhyd Ca2+ |
-1616 |
ΔHӨhyd F- |
-504 |
Which of the following is the correct value for the enthalpy change of solution, ΔHӨsol, of calcium fluoride, CaF2.
+531 kJ mol-1
+5275 kJ mol-1
+27 kJ mol-1
-1589 kJ mol-1
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Which compound would have the greatest difference between the theoretical and experimental value for lattice enthalpy?
AgCl
AgI
NaF
NaCl
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Which row correctly describes a reaction that is only feasible at a low temperature?
X (g) + Y (g) → Z (g) exothermic
R (s) → T (g) + U (g) endothermic
E (g) → 3F(g) endothermic
M (g) + 2N (g) → P (g) + Q (g) endothermic
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Use the data in the table to calculate the value of the first electron affinity of iodine
Name of enthalpy change |
Energy change (kJ mol-1) |
Enthalpy of atomisation of calcium |
+178 |
1st ionisation energy of calcium |
+590 |
2nd ionisation energy of calcium |
+1145 |
Enthalpy of atomisation of iodine |
+107 |
Lattice energy of calcium iodide |
-2074 |
Enthalpy of formation of calcium iodide |
-534 |
-294 kJ mol-1
-240 kJ mol-1
-480 kJ mol-1
-587 kJ mol-1
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Urea reacts with water to produce carbon dioxide and ammonia via the following reaction
CO(NH2)2 (aq) + H2O (l) → CO2 (g) + 2NH3 (g) ΔH = 133 kJ mol-1
Thermodynamic data for the components of this reaction are
Substance |
CO(NH2)2 (aq) |
H2O (l) |
CO2 (g) |
NH3 (g) |
Sꝋ (J K-1 mol-1) |
105 |
70 |
214 |
192 |
At which of the following temperatures will this reaction become feasible?
0.31 K
3.18 K
132.6 K
314 K
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Which of the following statements correctly explains the trend in enthalpy of hydration of the metal ions down Group 1?
The attraction between the ion and the hydrogen ions in water decreases down the group
The attraction the ion and the delta positive hydrogen atoms in water decreases down the group
The lone pair on the oxygen atom becomes more available for bonding
The attraction between the ion and the delta negative oxygen atoms in water decreases down the group
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