Free Printable PHY 306 Review Quiz

1.

Which of the followiing is an intensive variable of a thermodynamic system?

a)

mass

b)

entropy

c)

temperature

d)

volume

2.

_____ refers to the heat required to change the phase of a substance in a first-order phase transition.

a)

Latent Heat

b)

Fusion

c)

Specific Heat

d)

Sensible Heat

3.

The _____ law of thermodynamics is used to understand the concept of energy conservation.

a)

0th

b)

1st

c)

2nd

d)

3rd

4.

In an _____ thermodynamic process, there is no flow of heat between the system and the surroundings.

a)

isobaric

b)

isothermic

c)

adiabatic

d)

isochoric

5.

If the temperature of the heat source is increased, the efficiency of carnot heat engine _____.

a)

increases

b)

decreases

c)

remains constant

d)

increases first then becomes constant

6.

An ideal heat engine operates in Carnot's cycle between 227 $\degree C$ & 127 $\degree C$ . it absorbs $6.0\times10^{4\ }$ J of heat at high temperature. The amount of work is (a) .

7.

110 J of heat is added to a system. The change in the internal energy is 40 J.

Then the amount of work done is _____.

a)

150 J on the system

b)

70 J by the system

c)

150 J by the system

d)

70 J on the system

8.

In thermodynamics, which of the following is not a state function?

a)

Density

b)

Internal Energy

c)

Enthalpy

d)

Heat

9.

Heat does not spontaneously flow from a colder body to a hotter one. Which of the following thermodynamics law states this?

a)

Zeroth law of thermodynamics

b)

First law of thermodynamics

c)

Second law of thermodynamics

d)

Third law of thermodynamics

10.

The entropy of an isolated system can never _____.

a)

decrease

b)

be zero

c)

increase

11.

A definite area or space where the thermodynamic process takes place is known as the _____.

a)

thermodynamic system

b)

thermodynamic cycle

c)

thermodynamic equilibrium

d)

thermodynamic variable

12.

When two bodies are in thermal equilibrium with a third body, they are also in thermal equilibrium with

each other. This statement is called the _____.

a)

zeroth law of thermodyamics

b)

first law of thermodynamics

c)

second law of thermodynamics

d)

third law of thermodynamics

13.

A chemical reaction that releases heat is an _____.

a)

endothermic reaction

b)

exothermic reaction

14.

The value of $c_{V,m}$ for a diatomic gas is _____, if the vibrational motion is not considered.

a)

$\frac{3R}{2}$

b)

$\frac{5R}{2}$

c)

$\frac{7R}{2}$

d)

$\frac{9R}{2}$

15.

The value of the adiabatic index for a monaotomic gas is around (a) . (give your answer in 3 significant figures)

16.

What is the state of matter in the region of X?

a)

solid

b)

liquid

c)

gas

d)

supercritical fluid

17.

A system in which neither mass nor energy is exchanged with the surrounding is called a(an) _____.

a)

open system

b)

closed system

c)

isolated system

18.

A thermodynamic process in which the volume remain constant is called an _____.

a)

isochoric process

b)

isobaric process

c)

isentropic process

d)

isothermal process

19.

Under the constant temperature & pressure conditions, the chemical reaction proceeds spontaneously when _____.

a)

∆G > 0

b)

∆G < 0

c)

∆H > 0

d)

∆H< 0

20.

Which law of thermodynamics states that the absolute zero cannot be reached?

a)

1st

b)

2nd

c)

3rd

d)

0th

21.

A 7.50 L sealed jar at 17 °C contains 0.100 moles of oxygen & 0.200 moles of nitrogen gas. What is the pressure (in Pa) in the container? (3 significant figures for answer)

(a)

22.

Which of the following equation represents the Ideal Gas Law?

a)

b)

c)

d)

23.

Which state of H₂O has the greatest entropy?

a)

Ice

b)

Water

c)

Gas

d)

Same for all states

24.

The internal energy of a fixed mass of an ideal gas depends on the _____ only.

a)

pressure

b)

volume

c)

temperature

d)

mass

25.

According to the kinetic theory of matter, as the temperature of an object increases, its molecules _____.

a)

move faster

b)

get bigger

c)

move farther apart

d)

move faster & farther apart

e)

get bigger & farther apart

26.

Which of the following is NOT a path function?

a)

Internal energy

b)

Heat energy

c)

Work energy

d)

Entropy

27.

$\left(\frac{\partial T}{\partial V}\right)_{\mathrm{s}}$ =

a)

$-\left(\frac{\partial\mathrm{P}}{\partial S}\right)_{\mathrm{V}}$

b)

$\left(\frac{\partial\mathrm{P}}{\partial S}\right)_{\mathrm{V}}$

c)

$\left(\frac{\partial V}{\partial S}\right)_{\mathrm{P}}$

d)

$-\left(\frac{\partial V}{\partial S}\right)_{\mathrm{P}}$

28.

Given the following information, calculate the change of the standard Gibbs energy (in kJ) for the following chemical reaction at 25 ^oC. (2 significant figure for answer)

SnCl₄(l) + 2 H₂0 (l) $\Longleftrightarrow$ SnO₂(S) + 4 HCl (g)

ΔH⁰=+133.0 kJ and ΔS⁰ =+401.5 J/K

(a)

29.

Which of the following statements are CORRECT?

1. The first law of thermodynamics represents the principle of conservation of energy.

2. Room temperature is about 20 degrees on the Kelvin scale.

3. A calorie is approximately 4.2 J.

4. Heat has the same unit as work.

5. Heat is a temperature difference.

a)

1, 3, and 4.

b)

3 and 5.

c)

1 and 5.

d)

1, 2 and 3.

e)

2 and 4.

30.

Which one of the following statements is true?

a)

In an adiabatic process, the heat flow is positive

b)

In an isovolumetric process, the work done is positive

c)

The internal energy of a system is not a state function

d)

In a cyclic process, the change in internal energy is zero

e)

In an isobaric process, the change in internal energy is always zero

31.

The graph which is drawn to scale, shows two isotherms at temperatures of T and T₁ for a fixed mass of ideal gas. What is the relation between T₁ and T?

a)

T₁= $\frac{T}{2}$

b)

T₁= $\frac{T}{4}$

c)

T₁= 2T

d)

T₁= 4T

32.

The figure shows a complete cycle of change for an ideal gas. Heat enters the gas during the _____ stages.

a)

PQ and QR

b)

QR and RS

c)

RS and SP

d)

SP and QR

33.

1 mole of an ideal gas undergoes an adiabatic process, its temperature increases by ∆T and its volume changes by ∆V. Which of the following is correct?

a)

Pressure of the gas decreases

b)

Work done by gas is p∆V

c)

Internal energy increases by C_v,m∆T

d)

Heat flows out of the gas

34.

A monatomic gas expands adiabatically from the state X to the state Y as shown in the figure. What is the magnitude of the change in the internal energy (in kJ) of the gas?

(a)

35.

The variation of internal energy per mole U with temperature of a gas is shown in the graph. What is the adiabatic index? (give your answer in 3 significant figures)

(a)

36.

Temperature is a measure of the _____.

a)

total energy in a substance

b)

total kinetic energy in a substance

c)

average potential energy in a substance

d)

average kinetic energy of molecules in a substance

37.

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated with the same thermal energy from the same temperature. What material would be the coolest after being heated?

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

38.

Fermi-Dirac statistics is for the _____.

a)

distinguishable particles

b)

symmetrical Particles

c)

particles with half integral spin

d)

particles with integral spin

39.

Bose-Einstein statistics is for the _____.

a)

distinguishable particles

b)

symmetrical Particles

c)

particles with half integral spin

d)

particles with integral spin

40.

Maxwell-Boltzmann statistics is for the _____.

a)

distinguishable particles

b)

indistinguishable Particles

c)

particles with half integral spin

d)

particles with integral spin

41.

The average kinetic energy associated with each degree of freedom is _____.

a)

$k_BT$

b)

$2k_BT$

c)

$\frac{k_BT}{2}$

d)

$\frac{3k_BT}{2}$

42.

Which one of the following is the most probable speed?

a)

A

b)

B

c)

C

d)

D

43.

The difference between fermions and bosons is that bosons do not obey _____.

a)

Aufbau principle

b)

Pauli’s Exclusion Principle

c)

Hund’s Rule of Maximum Multiplicity

d)

Heisenberg’s Uncertainty Principle

44.

Striling’s approximation ln N! = _____.

a)

$N\ln N-N$

b)

$\frac{N}{2}\ln N+2$

c)

$N\ln N-1$

d)

$N\ln N+N$

45.

From the figure, what is the highest temperature?

a)

T1

b)

T2

c)

T3

d)

Insufficient information

46.

In Fermi-Dirac Statistics, one energy state can be occupied by more than one particle. This statement is _____.

a)

TRUE

b)

FALSE

47.

The ratio of rms velocity to most probable velocity is _____.

a)

$\sqrt[]{\frac{3}{2}}$

b)

$\sqrt[]{\frac{2}{3}}$

c)

$\sqrt[]{\frac{3\pi}{8}}$

d)

$\sqrt[]{\frac{\pi}{4}}$

48.

Which of the following is TRUE for a system that is in dynamic equilibrium?

a)

The forward reaction goes to 100% completion.

b)

The reaction stops.

c)

The concentration of products is equal to the concentration of the reactants.

d)

none of the above

49.

Le Chatelier's principle states that _____.

a)

a disturbing force must be applied to a system in order for it to reach equilibrium.

b)

when a system at equilibrium is disturbed, a new equilibrium constant is established.

c)

when a chemical system at equilibrium is disturbed, the system shifts in order to minimize the effect.

d)

when a chemical system is at equilibrium it is no longer possible to alter the system.

50.

What happens to the equilibrium position of an exothermic reaction when you remove heat?

a)

shifts to the left

b)

shifts to the right

c)

no change

d)

insufficient information

51.

For the reaction

SO₂ (g) + O₂ (g) ⇌ SO₃(g)

If the concentration of SO₂is increased, the equilibrium of the reaction will shift to the _____.

a)

left

b)

right

c)

right then left

d)

left then right

52.

For the reaction

N₂(g)+ 3 H₂(g) ⇌ 2 NH₃(g)

If the pressure in the system is increased, which substance(s) will increase in concentration?

a)

N₂

b)

H₂

c)

N₂ and H₂

d)

NH₃

53.

2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
Decreasing volume of container will _____.

a)

shift equilibrium to the right

b)

shift equilibrium to the left

c)

change $K_{eq}$

d)

have no change

54.

For a reaction $K_{eq}$ = 1.2 × 10^-6 at T = 200 K. What is ΔG° for the reaction in KJ / mol? (give your answer in 3 significant figures)

(a)

55.

A catalyst is added to a system at equilibrium. The concentration of the reactants will then _____.

a)

decrease

b)

increase

c)

remain the same

d)

approach zero

e)

none of the above

56.

The picture shows a reversible chemical reaction taking place. How can equilibrium be reached?

a)

Put a stopper on the flask.

b)

Add more reactants.

c)

Add more products.

d)

Cool the contents.

e)

Decrease the surrounding pressure.

57.

For the following chemical equilibrium, Kp = 4.6 × 10^-14 Pa at 25 °C, find the value of Kc (in $\frac{mol}{m^3}$ ) for this reaction at 25 °C.

2 Cl₂(g) + 2 H₂O (g) ⇔ 4 HCl (g) + O₂(g)

a)

Kc = 2.2 × 10^-14

b)

Kc = 4.6 × 10^-14

c)

Kc = 9.4 × 10^-14

d)

Kc = 1.9 × 10^-17

e)

Kc = 1.1 × 10^-12

58.

What is ΔH° (in kJ/mol) for a reaction that has $K_{eq}$ = 1.456 at 273 K and $K_{eq}$ = 14.2 at 298 K? (give your answer in 3 significant figures)

(a)

59.

What is the Kc expression for the reaction below:
SOCl₂ (g) + H₂O (g) ⇌ SO₂ (g) + 2 HCl (g)

a)

$\frac{[SO_2][2HCl]}{[SOCl_2][H_2O]}$

b)

$\frac{[SO_2][HCl]^2}{[SOCl_2][H_2O]}$

c)

$\frac{[SOCl_2][H_2O]}{[SO_2][2HCl]}$

d)

$\frac{[SOCl_2][H_2O]}{\left[[SO_2\right][2HCl]}$

60.

Using the phase transition diagram, which of the following states coexist at the same time on the red curve?

a)

solid and liquid

b)

solid and gas

c)

liquid and gas

d)

solid, liquid, and gas

61.

What letter on the diagram represents a substance only in the solid phase?

a)

A

b)

B

c)

C

d)

d

e)

e

62.

What letter on the diagram represents the triple point?

a)

A

b)

B

c)

C

d)

d

e)

e

63.

What is the boiling point of this substance at 1 atm of pressure?

a)

45 $\degree C$

b)

60 $\degree C$

c)

100 $\degree C$

d)

110 $\degree C$

64.

What would the state of this substance be at 0.5 ATM of pressure at a 100 $\degree C$ ?

a)

Solid

b)

Liquid

c)

Gas

d)

Liquid & gas coexist

e)

Solid & liquid coexist

65.

A phase change is a chemical or physical change?

a)

Physical

b)

Chemical

66.

Transition from solid to gas without the intermediate liquid phase is called _____.

a)

Condensation

b)

Vaporization

c)

Freezing

d)

Deposition

e)

Sublimation

67.

The pressure is increased on a sample of water at 0 °C from 0 mmHg to 800 mmHg. In order, what changes occur?

a)

deposition then melting

b)

sublimation then melting

c)

condensation then freezing

d)

vaporization then freezing

68.

What happens along the BC line?

a)

Melting or freezing

b)

Vaporization or condensation

c)

Vaporization or melting

d)

Freezing or condensation

e)

Sublimation or deposition

69.

The molecules of an ideal gas have _____.

a)

kinetic energy only

b)

potential energy only

c)

both kinetic energy and

potential energy

d)

no energy

70.

The van der Waals equation for 1 mole real gas is _____.

a)

$\left(P+\frac{a}{V^2}\right)\left(V-b\right)=RT$

b)

$\left(P+\frac{a}{nV^2}\right)=RT$

c)

$\left(P-\frac{a}{V^2}\right)\left(V+b\right)=RT$

d)

$PV=RT$

71.

The critical temperature of a van der Waals gas is _____.

a)

$T_C=\frac{8}{27bR}$

b)

$T_C=\frac{27}{8}\ \frac{a}{bR}$

c)

$T_C=\frac{a}{27b^2}$

d)

$T_C=\frac{8a}{27bR}$

72.

At high pressure, the real gas deviates from the ideal gas behavior, because _____.

a)

The gas molecules occupy sizable portion of the container.

b)

The intermolecular forces is significant as the molecules are now closer to each other.

c)

The molecule have energy to overcome intermolecular forces.

d)

The gas molecules move faster at high pressure.

73.

Based on the knowledge of Joule-Thomson effect, which of the following gases increase their temperature during the Joule-Thomson expansion?

a)

O₂& N₂

b)

H₂& He

c)

CO & O₂

d)

CH₄& N₂

74.

Oxygen molecules at temperature T have the same r.m.s. speed as helium molecules at 300 K. What is the temperature T in K?

(a)

75.

The change in length (in mm) of a 100 mm aluminium bar that has increased in temperature by 55 ⁰C.
Take the coefficient of linear expansion to be 2.5 x 10^-5 $K^{-1}$ . (give your answer in 2 significant figures)

(a)

76.

The mean free path is inversely proportional to the _____.

a)

density

b)

Pressure

c)

square of the diameter of the molecule

d)

All of the above

77.

$\left(\frac{\partial P}{\partial S}\right)_V$ equals to _____.

a)

$-\left(\frac{\partial V}{\partial T}\right)_P$

b)

$-\left(\frac{\partial T}{\partial V}\right)_S$

c)

$-\left(\frac{\partial P}{\partial T}\right)_V$

d)

$-\left(\frac{\partial T}{\partial V}\right)_S$

78.

Enthalpy H = _____.

a)

U + pV

b)

U + pdV

c)

dU+ pV

d)

pV

79.

A container having a volume of 1.0 m³ holds 5.0 moles of helium (He) gas at 50 °C. If the helium behaves like an ideal gas, what is the total energy of the system?

a)

2.0 × 10⁴ J

b)

2.5 × 10⁴ J

c)

1.7 × 10³ J

d)

1.5 × 10³ J

80.

A container having a volume of 1.0 m³ holds 5.0 moles of helium (He) gas at 50 °C. If the helium behaves like an ideal gas, the average kinetic energy per molecule is _____.

a)

3.3 × 10⁻²⁰ J

b)

1.0 × 10⁻²¹J

c)

1.0 × 10⁻²⁰J

d)

6.7 × 10⁻²¹ J

81.

The air in an automobile engine at 20.0 °C is compressed from an initial pressure of 1.00 atm and a volume of 200 cm³ to a volume of 20.0 cm³. Find the temperature (in K) if the air behaves like an ideal gas (γ = 1.40) and the compression is adiabatic. (give your answer in 3 significant figures)

(a)

82.

If $c_{p,m}$ for an ideal gas is 35.4 J/mol⋅K, which of the following is $c_{V,m}$ for this gas?

a)

12.5 J/mol⋅K

b)

20.8 J/mol⋅K

c)

29.1 J/mol⋅K

d)

27.1 J/mol⋅K

83.

For one phase and one component system, the degrees of freedom is _____.

a)

1

b)

2

c)

3

d)

4

84.

A system containing liquid water and water vapour has the number of phases equal to _____.

a)

2

b)

0

c)

1

d)

3

85.

What is meant by triple point?

a)

Degree of freedom is three

b)

Three phases are in equilibrium

c)

Three components are in equilibrium

86.

The ratio of the effusion speed of helium (He) to gas X is 16:1. What is the molar mass of gas X? (use 4 g/mol for He)

a)

1024 g/mol

b)

256 g/mol

c)

128 g/mol

d)

64 g/mol

87.

Effusion is _____.

a)

used to describe the combustibility of a gas

b)

the ability of a gas to escape through a tiny opening

c)

what occurs after diffusion.

d)

the ability of a gas to mix with other gases.

88.

A tank of gas contains 50 kPa of helium, 50 kPa of argon, and 100 kPa of neon. What is the total pressure (in kPa) of the gas mixture?

(a)

89.

What happens to the temperature of a substance during a phase change?

a)

Increases

b)

Remains constant

c)

Decreases

d)

Increases or Decreases

90.

A reversible and irreversible heat engines are working between same two temperatures .The efficiency of _____.

a)

both are the same

b)

the reversible is greater

c)

the irreversible is greater

91.

1200 J of heat are added to a sample of gas while the gas does 400 J of work on the environment. What is the change in internal energy (in J) of the gas?

(a)

92.

What is the correct form of equation for the first law of thermodynamics?

a)

$U=Q+W$

b)

$dU=Q+W$

c)

$\Delta U=\delta Q+dW$

d)

$dU=\delta Q-pdV$

e)

$dU=dQ+dW$

93.

COP of heat pump = COP of refrigerator + ____

a)

1

b)

4

c)

3

d)

2

94.

The cyclic integral of $\frac{\delta Q}{T}$ in a thermodynamic cycle can be _____ zero.

a)

greater than or equal to

b)

less than or equal to

c)

greater than

95.

A refrigerator needs to remove heat from 5 degree celsius cold body to a surrounding at 35 degree celsius. What is its COP? (give 2 significant figures for answer)

(a)

96.

A $1.0\ x\ 10^4$ m steel railroad track with a coefficient of linear expansion of $\frac{12\times10^{-6}}{K}$ changes temperature from $18\degree C$ to $40\degree C$ . By how many meters will the railroad tracks expand? (give 2 significant figures for answer)

(a)

97.

In which region(s) of the graph would we use a specific heat capacity to calculate heat energy?

a)

Region 1, 3, & 5

b)

Region 2 & 4

c)

Region 1 only

d)

Region 1 & 2

98.

In which region(s) of the graph would we use a latent heat to calculate heat energy?

a)

Region 1, 3, & 5

b)

Region 2 & 4

c)

Region 1 only

d)

Region 1 & 2

99.

Calculate the amount of heat (in MJ) required to convert 450 g of water at 100 ^oC to steam at the same temperature (Latent heat of vaporization of water = 22.7 x 10⁵ J/kg). (give 3 significant figures for answer)

(a)

100.

Consider the following reaction at a certain temperature.

2 SO₃(g) ⇌ 2 SO₂(g) + O₂(g)

When the initial concentration of SO₃(g) is 0.128 mol/m³, at equilibrium the concentration of oxygen gas is found to be 0.0130 mol/m³. Calculate Kc (in mol/m³). (give 3 significant figures for answer)

(a)

PHY 306 Review Quiz

Total questions: 100

Worksheet time: 2hrs 39mins

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