5) When a system ________, ΔE is always negative.

A) absorbs heat and does work

B) gives off heat and does work

C) absorbs heat and has work done on it

D) gives off heat and has work done on it

E) None of the above is always negative

B) gives off heat and does work

6) Which one of the following is an endothermic process?

A) ice melting

B) water freezing

C) boiling soup

D) Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases.

E) Both A and C

E) Both A and C

7) Which one of the following is an exothermic process?

A) ice melting

B) water evaporating

C) boiling soup

D) condensation of water vapor

E) Ammonium thiocyanate and barium hydroxide are mixed at 25 °C: the temperature drops.

D) condensation of water vapor

8) Of the following, which one is a state function?

A) H

B) q

C) w

D) heat

E) none of the above

A) H

9) Which of the following is a statement of the first law of thermodynamics?

A) E k =1/2 m_v²

B) A negative ΔH corresponds to an exothermic process.

C) ΔE = E final - E initial

D) Energy lost by the system must be gained by the surroundings.

E) 1 cal = 4.184 J (exactly)

D) Energy lost by the system must be gained by the surroundings.

10) The internal energy can be increased by ________.

(a) transferring heat from the surroundings to the system

(b) transferring heat from the system to the surroundings

(c) doing work on the system

A) a only

B) b only

C) c only

D) a and c

E) b and c

D) a and c

11) A ________ ΔH corresponds to an ________ process.

A) negative, endothermic

B) negative, exothermic

C) positive, exothermic

D) zero, exothermic

E) zero, endothermic

B) negative, exothermic

12) A ________ ΔH corresponds to an ________ process.

A) negative, endothermic

B) positive, exothermic

C) positive, endothermic

D) zero, exothermic

E) zero, endothermic

C) positive, endothermic

13) ΔH for an endothermic process is ________ while ΔH for an exothermic process is ________.

A) zero, positive

B) zero, negative

C) positive, zero

D) negative, positive

E) positive, negative

E) positive, negative

14) For a given process at constant pressure, w is positive. This means that the process involves ________.

A) work being done by the system on the surroundings

B) work being done by the surroundings on the system

C) no work being done

D) an equal amount of work done on the system and by the system

E) work being done against a vacuum

B) work being done by the surroundings on the system

15) Which one of the following statements is true?

A) Enthalpy is an intensive property.

B) The enthalpy change for a reaction is independent of the state of the reactants and products.

C) Enthalpy is a state function.

D) H is the value of q measured under conditions of constant volume.

E) The enthalpy change of a reaction is the reciprocal of the ΔH of the reverse reaction.

C) Enthalpy is a state function.

16) Which of the following statements is false ?

A) Internal energy is a state function.

B) Enthalpy is an intensive property.

C) The enthalpy change for a reaction is equal in magnitude, but opposite in sign, to the enthalpy change for the reverse reaction.

D) The enthalpy change for a reaction depends on the state of the reactants and products.

E) The enthalpy of a reaction is equal to the heat of the reaction.

B) Enthalpy is an intensive property.

17) A chemical reaction that absorbs heat from the surroundings is said to be ________ and has a ________ ΔH at constant pressure.

A) endothermic, positive

B) endothermic, negative

C) exothermic, negative

D) exothermic, positive

E) exothermic, neutral

A) endothermic, positive

18) A chemical reaction that releases heat to the surroundings is said to be ________ and has a ________ ΔH at constant pressure.

A) endothermic, positive

B) endothermic, negative

C) exothermic, negative

D) exothermic, positive

E) exothermic, neutral

C) exothermic, negative

9) The reaction

4Al (s) + 3O₂ (g) → 2Al 2 O₃ (s) ΔH° = -3351 kJ

is ________, and therefore heat is ________ by the reaction.

A) endothermic, released

B) endothermic, absorbed

C) exothermic, released

D) exothermic, absorbed

E) thermoneutral, neither released nor absorbed

C) exothermic, released

20) Under what condition(s) is the enthalpy change of a process equal to the amount of heat transferred into or out of the system?

(a) temperature is constant

(b) pressure is constant

(c) volume is constant

A) a only

B) b only

C) c only

D) a and b

E) b and c

B) b only

21) The units of heat capacity are ________.

A) K/J or °C/J

B) J/K or J/°C

C) J/g-K or J/g-°C

D) J/mol

E) g-K/J or g-°C/J

B) J/K or J/°C

22) The units of specific heat are ________.

A) K/J or °C/J

B) J/K or J/°C

C) J/g-K or J/g-°C

D) J/mol

E) g-K/J or g-°C/J

C) J/g-K or J/g-°C

23) The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1 °F. There are ________ Btu in one Joule. 1 lb = 453.59 g; °C = (5/9)(°F - 32°); specific heat of H 2 O (l) = 4.184 J/g-K.

A) 1056 Btu

B) 1.896 × 10 -3 Btu

C) 9.278 × 10 -4 Btu

D) 5.120 × 10 -3 Btu

E) Additional information is needed to complete the calculation.

C) 9.278 × 10 -4 Btu

24) Which of the following is a statement of Hess's law?

A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps.

B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps.

C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction.

D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction.

E) The ΔH of a reaction depends on the physical states of the reactants and products.

A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps.

25) For which one of the following reactions is ΔH° rxn equal to the heat of formation of the product?

A) N₂ (g) + 3H₂ (g) → 2NH₃ (g)

B) (1/2)N₂ (g) + O₂ (g) → NO₂ (g)

C) 6C (s) + 6H (g) → C₆ H₆ (l)

D) P (g) + 4H (g) + Br (g) → PH₄ Br (l)

E) 12C (g) + 11H₂ (g) + 11O (g) → C₆ H₂₂ O₁₁ (g)

B) (1/2)N₂ (g) + O₂ (g) → NO₂ (g)

26) Of the following, ΔH° f is not zero for ________.

A) O₂ (g)

B) C (graphite)

C) N₂ (g)

D) F₂ (s)

E) Cl₂ (g)

D) F₂ (s)

27) Of the following, ΔH° f is not zero for ________.

A) Sc (g)

B) Si (s)

C) P 4 (s, white)

D) Br 2 (l)

E) Ca (s)

A) Sc (g)

28) Consider the following two reactions:

A → 2B ΔH° rxn = 456.7 kJ/mol

A → C ΔH° rxn = -22.1 kJ/mol

Determine the enthalpy change for the process:

2B → C

A) -478.8 kJ/mol

B) -434.6 kJ/mol

C) 434.6 kJ/mol

D) 478.8 kJ/mol

E) More information is needed to solve the problem.

A) -478.8 kJ/mol

29) In the reaction below, ΔH° f is zero for ________.

Ni (s) + 2CO (g) + 2PF 3 (g) → Ni(CO) 2 (PF 3 ) 2 (l)

A) Ni (s)

B) CO (g)

C) F 3 (g)

D) Ni(CO) 2 (PF 3 ) 2 (l)

E) both CO (g) and PF 3 (g)

A) Ni (s)

30) For the species in the reaction below, ΔH° f is zero for ________.

2Co (s) + H 2 (g) + 8PF 3 (g) → 2HCo(PF 3 ) 4 (l)

A) Co (s)

B) H 2 (g)

C) PF 3 (g)

D) HCo(PF 3 ) 4 (l)

E) both Co(s) and H 2 (g)

E) both Co(s) and H 2 (g)

31) For which one of the following equations is ΔH° rxn equal to ΔH° f for the product?

A) Xe (g) + 2F 2 (g) → XeF 4 (g)

B) CH 4 (g) + 2Cl 2 (g) → CH 2 Cl 2 (l) + 2HCl (g)

C) N 2 (g) + O 3 (g) → N 2 O 3 (g)

D) 2CO (g) + O 2 (g) → 2CO 2 (g)

E) C (diamond) + O 2 (g) → CO 2 (g)

A) Xe (g) + 2F 2 (g) → XeF 4 (g)

32) For which one of the following reactions is the value of ΔH° rxn equal to ΔH° f for the product?

A) 2Ca (s) + O 2 (g) → 2CaO (s)

B) C 2 H 2 (g) + H 2 (g) → C 2 H 4 (g)

C) 2C (graphite) + O 2 (g) → 2CO (g)

D) 3Mg (s) + N 2 (g) → Mg 3 N 2 (s)

E) C (diamond) + O 2 (g) → CO 2 (g)

D) 3Mg (s) + N 2 (g) → Mg 3 N 2 (s)

33) For which one of the following reactions is the value of ΔH° rxn equal to ΔH° f for the product?

A) 2C (s, graphite) + 2H 2 (g) → C 2 H 4 (g)

B) N 2 (g) + O 2 (g) → 2NO (g)

C) 2H 2 (g) + O 2 (g) → 2H 2 O (l)

D) 2H 2 (g) + O 2 (g) → 2H 2 O (g)

E) H 2 O (l) + 1/2 O 2 (g) → H 2 O 2 (l)

A) 2C (s, graphite) + 2H 2 (g) → C 2 H 4 (g)

34) For which one of the following reactions is the value of ΔH° rxn equal to ΔH° f for the product?

A) H 2 O (l) + 1/2 O 2 (g) → H 2 O 2 (l)

B) N 2 (g) + O 2 (g) → 2NO (g)

C) 2H 2 (g) + O 2 (g) → 2H 2 O (l)

D) 2H 2 (g) + O 2 (g) → 2H 2 O (g)

E) none of the above

E) none of the above

35) Fuel values of hydrocarbons increase as the H/C atomic ratio increases. Which of the following compounds has the highest fuel value?

A) C 2 H 6

B) C 2 H 4

C) C 2 H 2

D) CH 4

E) C 6 H 6

D) CH 4

36) Of the substances below, the highest fuel value is obtained from ________.

A) charcoal

B) bituminous coal

C) natural gas

D) hydrogen

E) wood

D) hydrogen

37) Which one of the choices below is not considered a fossil fuel?

A) anthracite coal

B) crude oil

C) natural gas

D) hydrogen

E) petroleum

D) hydrogen

38) The most abundant fossil fuel is ________.

A) natural gas

B) petroleum

C) coal

D) uranium

E) hydrogen

C) coal

39) Calculate the kinetic energy in J of an electron moving at 6.00 × 10 6 m/s. The mass of an electron is
9.11 × 10 -28 g.

A) 4.98 × 10 -48 J

B) 3.28 × 10 -14 J

C) 1.64 × 10 -17 J

D) 2.49 × 10 -48 J

E) 6.56 × 10 -14 J

C) 1.64 × 10 -17 J

40) The kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s is ________ J.

A) 1.2 × 10 3

B) 66

C) 2.4 × 10 3

D) 1.3 × 10 2

E) 7.3

A) 1.2 × 10 3

41) Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.

A) 3.60 × 10 6 J

B) 1.20 × 10 4 J

C) 3.60 × 10 3 J

D) 12.0 J

E) 80.0 J

A) 3.60 × 10 6 J

42) The ΔE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is
________ J.

A) 16.6

B) 12.4

C) 4.2

D) -16.6

E) -8.2

D) -16.6

43) The ΔE of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is
________ J.

A) 16.6

B) 12.4

C) 4.2

D) -16.6

E) 8.2

E) 8.2

44) The value of ΔH° for the reaction below is -1107 kJ:

2Ba (s) + O 2 (g) → 2BaO (s)

How many kJ of heat are released when 5.75 g of BaO (s) is produced?

A) 56.9 kJ

B) 23.2 kJ

C) 20.8 kJ

D) 193 kJ

E) 96.3 kJ

C) 20.8 kJ

45) The value of ΔH° for the reaction below is -1107 kJ:

2Ba (s) + O 2 (g) → 2BaO (s)

How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?

A) 20.8 kJ

B) 63.5 kJ

C) 114 kJ

D) 70.3 kJ

E) 35.1 kJ

B) 63.5 kJ

46) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?

A) 2.0 J

B) -0.13 J

C) 5.8 × 10 -4 J

D) 29 J

E) 0.13 J

D) 29 J

47) The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is ________ J/g-K.

A) 7.8

B) 1.9

C) 29

D) 0.13

E) -29

D) 0.13

48) The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K) of bromine liquid is ________.

A) 707 J/mol-K

B) 36.1 J/mol-K

C) 18.1 J/mol-K

D) 9.05 J/mol-K

E) 0.226 J/mol-K

B) 36.1 J/mol-K

50) ΔH for the reaction

IF 5 (g) → IF 3 (g) + F 2 (g)

is ________ kJ, give the data below.

IF (g) + F 2 (g) → IF 3 (g) ΔH = -390 kJ

IF (g) + 2F 2 (g) → IF 5 (g) ΔH = -745 kJ

A) +355

B) -1135

C) +1135

D) +35

E) -35

A) +355

51) Given the following reactions

Fe 2 O 3 (s) + 3CO (s) → 2Fe (s) + 3CO 2 (g) ΔH = -28.0 kJ

3Fe (s) + 4CO 2 (s) → 4CO (g) + Fe 3 O 4 (s) ΔH = +12.5 kJ

the enthalpy of the reaction of Fe 2 O 3 with CO

3Fe 2 O 3 (s) + CO (g) → CO 2 (g) + 2 Fe 3 O 4 (s)

is ________ kJ.

A) -59.0

B) 40.5

C) -15.5

D) -109

E) +109

A) -59.0

52) Given the following reactions

N 2 (g) + 2O 2 (g) → 2NO 2 (g) ΔH = 66.4 kJ

2NO (g) + O 2 (g) → 2NO 2 (g) ΔH = -114.2 kJ

the enthalpy of the reaction of the nitrogen to produce nitric oxide

N 2 (g) + O 2 (g) → 2NO (g)

is ________ kJ.

A) 180.6

B) -47.8

C) 47.8

D) 90.3

E) -180.6

A) 180.6

53) Given the following reactions

2S (s) + 3O 2 (g) → 2SO 3 (g) ΔH = -790 kJ

S (s) + O 2 (g) → SO 2 (g) ΔH = -297 kJ

the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide

2SO 2 (g) + O 2 (g) → 2SO 3 (g)

is ________ kJ.

A) 196

B) -196

C) 1087

D) -1384

E) -543

B) -196