WorksheetsCollege Chemistry Unit 8 Lessons 2 Practice
Total questions: 15
Worksheet time: 24mins
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
How do you calculate Enthalpy of a reaction?
ΔH = ΔHproducts - ΔHreactants
ΔT = q / mC
ΔG = ΔH -TΔS
E = mc2
Which of the following has a ΔHfo value of 0?
Br2(g)
N(g)
CO(g)
N2(g)
Which of the equations 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
How much heat is required to raise the temperature of 18.8 g of copper from 10.0°C to 75.0°C?The specific heat of copper is 0.385 J/g·°C.
3174.0 J
8.98 J
542.9 J
470.5 J
Use the information in the image to answer this question.
The standard enthalpy of combustion of butane, in kJ mol−1, is
C4H10(g) + 6.5O2(g) --> 4CO2(g) + 5H2O(l)
−2880 kJ
−2590 kJ
−806 kJ
−554 kJ
The standard enthalpy changes of combustion of carbon, hydrogen and methane are shown in the table.
What is the standard enthalpy change of formation of methane in kJ mol–1?
C(s) + 2H2(g) → CH4(g)
+211 kJ
-211 kJ
+75 kJ
-75 kJ
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 kJ
130 kJ
-130 kJ
-910 kJ
Using the equations below
Cu(s) + 1/2O2(g) → CuO(s) ∆H = –156 kJ
2Cu(s) + O2(g) → Cu2O(s) ∆H = –170 kJ
What is the value of ∆H (in kJ) for the following reaction?
2CuO(s) → Cu2O(s) + 1/2O2(g)
142 kJ
-482 kJ
14 kJ
-142 kJ
You are given these two equations:
2H2 + O2 → 2H2O ∆H = -572 kJ
H2 + O2 → H2O2 ∆H = -188 kJ
∆H = -948 kJ
∆H = -196 kJ
∆H = -384 kJ
∆H = -188 kJ
What is the Heat of Reaction ΔH for this reaction?
-200 KJ
200 KJ
400 KJ
-300 KJ
What type of reaction is this?
Exothermic
Endothermic
Energy Producing
No way to tell
What type of reaction is this?
Exothermic
Endothermic
Energy Producing
No way to tell
What is the Heat of Reaction ΔH for this reaction?
+50 KJ
-50 KJ
-100 KJ
+100 KJ
