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WorksheetsENTHALPY
Total questions: 17
Worksheet time: 4hrs 15mins
Match the definition below to the correct term.
The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.
The enthalpy of neutralisation
The enthalpy of combustion
The enthalpy of formation
The enthalpy of reaction
Name the type of enthalpy for the following reaction:
Na+ (g) --> Na+ (aq) ΔH = -364 kJmol-1
Standard enthalpy of neutralisation, ΔHneuto
Standard enthalpy of solution, ΔHsolno
Standard enthalpy of hydration, ΔHhydo
lattice energy, ΔHlatticeo
Which of the following has a ΔHfo value of 0?
Br2(g)
N(g)
CO(g)
N2(g)
Which of the equation below refers to the standard enthalpy of formation, ΔHfo?
Na(g) ---> Na+(g) + e- ΔH = -364 kJmol-1
C2H5OH(l) + 3O2(g) ---> 2CO2(g) + 3H2O (l) ΔH = - 1286 kJmol-1
2C(s) + 2H2(g) ---> C2H4 (g) ΔH = - 52.3 kJmol-1
Na+(g) ---> Na+(aq) ΔH = - 364 kJmol-1
The specific heat of copper is 0.39 J/g °C. What is the temperature change when 100 Joules of heat is added to 20 grams?
12.82 °C
24.12°C
351 °C
Using the equations below:
C(s) + O2(g) → CO2(g) ∆H = –390 kJ
Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ
what is ∆H (in kJ) for the following reaction?
MnO2(s) + C(s) → Mn(s) + CO2(g)
910
130
-130
-910
Which of the following statements are true for the reaction:
SO2(g) + 1/2O2(g) ↔ SO3(g) ΔH = –92 kJ mol-1
Where ↔ indicates that the reaction can proceed in the forward and the reverse direction.
The forward and reverse reaction both produce 92 kJ of energy.
Oxidising 2 moles of SO2 would produce twice as much energy.
The reverse reaction has an enthalpy of +92 kJ mol-1.
Collecting the SO3 produced in the liquid state would not change the measured enthalpy.
In order to find the enthalpy of combustion of C3H8 how must the enthalpy changes be arranged?
ΔH3 = ΔH1 + ΔH2
ΔH2 = ΔH3 - ΔH1
ΔH1 = ΔH2 - ΔH3
0 = ΔH1 + ΔH2 + ΔH3
The standard enthalpy change of formation values of two oxides of phosphorus are:
P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1
P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1
What is the enthalpy change, in kJ mol–1, for the reaction below?
P4O6(s) + 2O2(g) → P4O10(s)
+4600
+1400
–1400
–4600
Which of the following represent enthalpy change of solution?
Cl2(g) + (aq) ---> 2Cl-(aq) .
Mg2+(g) ---> Mg2+(aq)
MgCl2(s) + (aq) ---> Mg2+(aq) + 2Cl-(aq) .
Mg2+(g) + 2Cl-(g) + (aq) --> Mg2+(aq) + 2Cl-(aq)
Which of the following equations represents the enthalpy change of combustion?
2C4H10(g) +13O2(g) → 8CO2 (g) + 10H20(g)
C4H10(g) +13/2O2(g) → 4CO2 (g) + 5H20(g)
C4H10 + 9/2O2 = 4CO (s)+ 5H2O
C4H10 + 5/2O2 = 4C(s) + 5H2O(g)
At 550 °C nitrogen dioxide reacts with unburnt hydrocarbon fragments such as CH3 in the catalytic converter of a motor vehicle.
4CH3 + 7NO2 → 3.5N2 + 4CO2 + 6H2O
Which row gives the energy change for this reaction and a possible reason for it?
A
B
C
D
An important reaction in the manufacture of nitric acid is the catalytic oxidation of ammonia.
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
For every mole of O2 that reacts in this way, 181.8 kJ of energy are released.
A factory makes 2.50 × 105 mol of NO every day.
How much energy, in kJ, is released every day?
3.64 × 107
4.55 × 107
5.68 × 107
2.27 × 108
