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Thermochemistry

Total questions: 46

Worksheet time: 38mins

Name
Class
Date
1.

The enthalpy of formation is the enthalpy change

a)

when one mole of the pure compound is formed from its elements under standard conditions

b)

when 1 mole of pure substance is completely burned in excess oxygen, under the given temperature and pressure of the reaction

c)

when 1 mole of H+ (aq) ions from acid reacts with 1 mole of OH- (aq) ions from an alkali to form 1 mole of water under the stated condition of the experiment

d)

the magnitude of the enthalpy change of a chemical reaction depends only on the difference in the enthalpy content of the products and the reactants, and does not on how the reaction is completed

2.

Which of the following equations represents the enthalpy change of combustion?

a)

2C4H10(g) +13O2(g) → 8CO2 (g) + 10H20(g)

b)

C4H10(g) +13/2O2(g) → 4CO2 (g) + 5H20(g)

c)

C4H10 + 9/2O2 = 4CO (s)+ 5H2O

d)

C4H10 + 5/2O2 = 4C(s) + 5H2O(g)

3.

What does the circle mean in ΔH°?

a)

Standard Conditions (T=298.15 K P=1 atm)

b)

Standard Temperature and Pressure (T=273.15 K P=1 atm)

c)

Degree K

d)

Degree C

4.

"Heat change when 1 mole of gaseous atom is formed from its element at standard states" is the definition for _______.

a)

standard enthalpy of formation

b)

standard enthalpy ofhydration

c)

electron affinity

d)

standard enthalpy of atomisation

5.
Calorimetry is a technique used to
a)
measure temperature change
b)
measure heat released
c)
measure heat absorbed
d)
measure the enthalpy change for a reaction
6.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
7.

Enthalpy of Atomisation is heat absorbed when ____________ atom is formed from its element at their stated states

a)

1 mol of compound

b)

1 mol of substance

c)

1 mol of gaseous atom

d)

1 mol of water

8.

Which of the reaction is enthalpy of atomisation?

a)

Na(g) --> Na(g)

b)

Na(s) --> Na(g)

c)

Na(g) --> Na(s)

d)

Na(s) --> Na(s)

9.

Which one of the following enthalpy of formation is zero?

a)

Enthalpy formation of H2O (l)

b)

Enthalpy formation of H2(g)

c)

Enthalpy formation of NaCl(s)

d)

Enthalpy formation of CH4(g)

10.

The transfer of energy from one state to another at constant pressure is called...

a)

Calories

b)

Work

c)

Enthalpy

d)

Potential energy

e)

Kinetic energy

11.

Name the following Ionic Compound:

KCl

a)

Potassium Chlorine

b)

Potassium (I) Chlorine

c)

Potassium (II) Chloride

d)

Potassium Chloride

12.
Conditions for standard enthalpy change are
a)
Temp-298K, Press - 100kPa, Conc-1M
b)
Temp-273K, Press - 100Pa, Conc-1M
c)
Temp-298K, Press - 100Pa, Conc-1M
d)
Temp-273K, Press - 100kPa, Conc-1M
13.
Diagram below shows
a)
Standard lattice enthalpy
b)
Standard enthalpy of solution
c)
Standard enthalpy of formation
d)
Standard enthalpy of hydration
14.
Diagram below shows
a)
Standard lattice enthalpy
b)
Standard enthalpy of precipitation
c)
Standard enthalpy of formation
d)
Standard enthalpy of hydration
15.

Which of the following represent the enthalpy change of atomization?

a)

O2(g) → 2 O(g)

b)

Mg(s) → Mg(g)

c)

Mg(s) + Cl2(g) → MgCl2(s)

d)

Ca(g) → Ca2+(g) + 2 e

16.

which of the following enthalpy changes represent the enthalpy change of formation?

a)

Mg(s) + Cl2(g) → MgCl2(s)

b)

Mg2+(g) + 2 Cl -(g) → MgCl2(aq)

c)

O2(g) → 2 O(g)

d)

2Mg (s) + O2(g) → 2MgO(S)

17.

Which one represent the electron affinity of chlorine?

a)

1/2Cl2(g) → 2 Cl(g)

b)

Cl(g) + e → Cl- (g)

c)

1/2 Cl2(g) + e → Cl- (g)

d)

Cl2(g)→ 2 Cl-(g) + 2e-

18.

which of the following represent the enthalpy change of 1st ionization enthalpy?

a)

Mg(s) --> Mg2+(g) + 2e-(aq)

b)

Mg(s) --> Mg+(g) + e-(aq)

c)

Mg(s) --> Mg+(g) + e-(aq)

d)

Mg(g) --> Mg+(g) + e-(aq)

19.

MgCl2(s) ---> Mg2+(g) + 2Cl-(g)

This equation represents

a)

Enthalpy of hydration

b)

Enthalpy of solution

c)

Lattice enthalpy of dissociation

d)

Lattice enthalpy of formation

20.

1/2 O2(g) → O(g)

This equation represents.

a)

Enthalpy of atomization

b)

enthalpy of sublimation

c)

enthalpy of dissociation

d)

enthalpy of formation

21.

which of the following represent the equation for enthalpy of sublimation

a)

1/2 Br (s) → Br(g)

b)

1/2 I 2(s) → I(g)

c)

1/2 O(g) → 2 O(g)

d)

Mg(s) → Mg2+ (g) + 2e

22.

Which of the ionic compounds has the highest lattice energy

a)

NaBr

b)

KF

c)

KI

d)

NaF

23.

4Al(s) + 3O2(g) →  2Al2O3(s)   ΔH =−3352 kJ 4Al\left(s\right)\ +\ 3O_2\left(g\right)\ \rightarrow\ \ 2Al_2O_3\left(s\right)\ \ \ \Delta H\ =-3352\ kJ\ ^{ }  

Calculate the enthalpy change to produce 4 moles of Al2O3Al_2O_3  

a)

-1676

b)

-6704 kJ

c)

-13408 kJ

d)

-3352 kJ

24.

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)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

25.
(Hess's Law)Calculate the ∆H for the following reaction: 2H2O2 →  2H2O  + 1 O2 
You are given these two equations:
2H2  +  O2 → 2H2O            ∆H  =  -572 kJ
 H2  +  O2  →  H2O2            ∆H  =  -188 kJ 
a)
∆H  =  -948 kJ 
b)
∆H  =  -196 kJ 
c)
∆H  =  -384 kJ 
d)
∆H  =  -188 kJ 
26.

What is the enthalpy of formation of buta-1,3-diene, C4H6(g)?

a)

+112 kJ mol–1

b)

–112 kJ mol–1

c)

+746 kJ mol–1

d)

–746 kJ mol–1

27.

Which enthalpy change Symbol best represents this reaction?


Br-(g) → Br-(aq)

a)

∆Hθhyd

b)

∆Hθc

c)

∆Hθr

d)

∆Hθsol

28.

Which enthalpy change Symbol best represents this reaction?


HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)

a)

∆Hθf

b)

∆Hθhyd

c)

∆Hθr

d)

∆Hθn

29.

Which enthalpy change Symbol best represents this reaction?


Sn(s) + S(s) + 2O2(g) → SnSO4(s)

a)

∆Hθc

b)

∆Hθf

c)

∆Hθr

d)

∆Hθsol

30.

Which of the following represent the enthalpy change of atomization?

a)

O2(g) → 2 O(g)

b)

Mg(s) → Mg(g)

c)

Mg(s) + Cl2(g) → MgCl2(s)

d)

Ca(g) → Ca2+(g) + 2 e

31.

Which one represent the electron affinity of chlorine?

a)

1/2Cl2(g) → 2 Cl(g)

b)

Cl(g) + e → Cl- (g)

c)

1/2 Cl2(g) + e → Cl- (g)

d)

Cl2(g)→ 2 Cl-(g) + 2e-

32.

Which of the following represent enthalpy change of solution?

a)

Cl2(g) + (aq) ---> 2Cl-(aq) .

b)

Mg2+(g) ---> Mg2+(aq)

c)

MgCl2(s) + (aq) ---> Mg2+(aq) + 2Cl-(aq) .

d)

Mg2+(g) + 2Cl-(g) + (aq) --> Mg2+(aq) + 2Cl-(aq)

33.

which of the following represent the enthalpy change of 1st ionization enthalpy?

a)

Mg(s) --> Mg2+(g) + 2e-(aq)

b)

Mg(s) --> Mg+(g) + e-(aq)

c)

Mg(s) --> Mg+(g) + e-(aq)

d)

Mg(g) --> Mg+(g) + e-(aq)

34.

MgCl2(s) ---> Mg2+(g) + 2Cl-(g)

This equation represents

a)

Enthalpy of hydration

b)

Enthalpy of solution

c)

Lattice enthalpy of dissociation

d)

Lattice enthalpy of formation

35.

1/2 O2(g) → O(g)

This equation represents.

a)

Enthalpy of atomization

b)

enthalpy of sublimation

c)

enthalpy of dissociation

d)

enthalpy of formation

36.

which of the following represent the equation for enthalpy of sublimation

a)

1/2 Br (s) → Br(g)

b)

1/2 I 2(s) → I(g)

c)

1/2 O(g) → 2 O(g)

d)

Mg(s) → Mg2+ (g) + 2e

37.

which of the following represent the lattice enthalpy of formation of sodium flouride

a)

2Na(g) + F2(g) → 2NaF(g)

b)

Na(s) + 1/2F2(g) → NaF(s)

c)

2Na(s) + 1/2F2(g) → NaF(g)

d)

2Na(s) + F2(g) → 2NaF(g)

38.

Which of the following equations represents the enthalpy change of combustion?

a)

2C4H10(g) +13O2(g) → 8CO2 (g) + 10H20(g)

b)

C4H10(g) +13/2O2(g) → 4CO2 (g) + 5H20(g)

c)

C4H10 + 9/2O2 = 4CO (s)+ 5H2O

d)

C4H10 + 5/2O2 = 4C(s) + 5H2O(g)

39.

which of the following enthalpy changes represent the enthalpy change of formation?

a)

Mg(s) + Cl2(g) → MgCl2(s)

b)

Mg2+(g) + 2 Cl -(g) → MgCl2(aq)

c)

O2(g) → 2 O(g)

d)

2Mg (s) + O2(g) → 2MgO(S)

40.

which of the following represent the enthalpy change of hydration?

a)

Mg(s) → Mg2+(g)

b)

Mg(s) → Mg2+(g) + 2 e

c)

Cl2(g) + (aq)→ 2Cl(aq)

d)

Mg(g) +(aq) → Mg2+(aq)

41.

which of the following enthalpy changes represent the enthalpy change of formation?

a)

Mg(s) + Cl2(g) → MgCl2(s)

b)

Mg2+(g) + 2 Cl -(g) → MgCl2(aq)

c)

O2(g) → 2 O(g)

d)

2Mg (s) + O2(g) → 2MgO(S)

42.

Which one represent the electron affinity of chlorine?

a)

1/2Cl2(g) → 2 Cl(g)

b)

Cl(g) + e → Cl- (g)

c)

1/2 Cl2(g) + e → Cl- (g)

d)

Cl2(g)→ 2 Cl-(g) + 2e-

43.

which of the following represent the enthalpy change of 1st ionization enthalpy?

a)

Mg(s) --> Mg2+(g) + 2e-(aq)

b)

Mg(s) --> Mg+(g) + e-(aq)

c)

Mg(s) --> Mg+(g) + e-(aq)

d)

Mg(g) --> Mg+(g) + e-(aq)

44.

MgCl2(s) ---> Mg2+(g) + 2Cl-(g)

This equation represents

a)

Enthalpy of hydration

b)

Enthalpy of solution

c)

Lattice enthalpy of dissociation

d)

Lattice enthalpy of formation

45.

which of the following represent the lattice enthalpy of formation of sodium flouride

a)

2Na(g) + F2(g) → 2NaF(g)

b)

Na(s) + 1/2F2(g) → NaF(s)

c)

2Na(s) + 1/2F2(g) → NaF(g)

d)

2Na(s) + F2(g) → 2NaF(g)

46.

Which of the following equations represents the enthalpy change of combustion?

a)

2C4H10(g) +13O2(g) → 8CO2 (g) + 10H20(g)

b)

C4H10(g) +13/2O2(g) → 4CO2 (g) + 5H20(g)

c)

C4H10 + 9/2O2 = 4CO (s)+ 5H2O

d)

C4H10 + 5/2O2 = 4C(s) + 5H2O(g)

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