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WorksheetsThermochemistry
Total questions: 21
Worksheet time: 32mins
The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?
#1 represents the enthalpy change for this exothermic reaction.
#2 represents the enthalpy change for this endothermic reaction.
#3 represents the enthalpy change for this endothermic reaction.
#4 represents the enthalpy change for this exothermic reaction.
The reaction of calcium chloride and water in the hot pack
tindak balas antara kalsium klorida dengan air dalam pek panas
releases water/ membebaskan air
releases heat/ membebaskan haba
absorbs water/ menyerap air
absorbs heat/ menyerap haba
A student must use 225 g of hot water in a lab procedure. If the specific heat of water is 4.184 J/g°C Calculate the amount of heat required to raise the temperature of water from 20.0 C to 100.0 C.
94140 J
75312 J
18828 J
0.672 J
The specific heat of a substance (C), whose units are J/g°C, is defined as
The number of Joules required to raise the temperature of 1 gram of the substance 1 °C.
The change in temperature when you add 1 Joule of energy.
The number of grams created when the substance cools down 1°C.
How hot or cold that specific amount of substance is.
Is the following change of state an endothermic process or an exothermic process? H2O(l) + E --> H2O(g)
Exothermic
Endothermic
Neither endothermic or exothermic
Both endothermic and exothermic
According to the diagram, what is ΔH for the reaction?
80 kJ
-80 kJ
240 kJ
-160 kJ
What is the specific heat of a 230 g metal that takes 3.1 kcal to heat from 25 *C to 83*C
0.0023 cal /g *C
0.23 cal /g *C
3400 cal /g *C
3.4 cal / g*C
How much energy must be used to produce 4.75 mol of gaseous water?
H2O (l) + 44.0 kJ --> H2O (g)
209 kJ
9.26 kJ
206 kJ
9.36 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
130
-130
-910
The following equations show the oxidation of carbon and carbon monoxide to carbon dioxide.
C(s) +O2(g) → CO2(g) ΔH = –x kJ mol–1
CO(g) + O2(g) → CO2(g) ΔH = –y kJ mol–1
What is the enthalpy change, in kJ mol–1, for the oxidation of carbon to carbon monoxide?
C(s) + O2(g) → CO(g)
x + y
-x - y
y - x
x - y
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
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
Which of the following represent the enthalpy change of atomization?
O2(g) → 2 O(g)
Mg(s) → Mg(g)
Mg(s) + Cl2(g) → MgCl2(s)
Ca(g) → Ca2+(g) + 2 e
which of the following represent the enthalpy change of hydration?
Mg(s) → Mg2+(g)
Mg(s) → Mg2+(g) + 2 e
Cl2(g) + (aq)→ 2Cl(aq)
Mg2+(g) → Mg2+(aq)
MgCl2(s) ---> Mg2+(g) + 2Cl-(g)
This equation represents
Enthalpy of hydration
Enthalpy of solution
Lattice enthalpy of dissociation
Lattice enthalpy of formation
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)
How do you calculate the Enthalpy of Reaction?
ΔH = ΔHproducts - ΔHreactants
ΔG = ΔH -TΔS
ΔT = q / mC
E = mc2
Hfinal > Hinitial means _____
change of enthalpy is positive and system absorbs heat
change of enthalpy is negative and system absorbs heat
change of enthalpy is positive and system loses heat
change of enthalpy is negative and system loses heat
