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Thermo

Total questions: 160

Worksheet time: 40hrs 0mins

Name
Class
Date
1.

The equation for heat transfer is  ΔQ = m×c×ΔT\Delta Q\ =\ m\times c\times\Delta T  What is represented by  ΔQ\Delta Q  ?

a)

heat, measured in calories

b)

mass, measured in grams

c)

specific heat, in calories/gram/degree C

d)

temperature change in degree C

2.

The equation for heat transfer is  ΔQ = m×c×ΔT\Delta Q\ =\ m\times c\times\Delta T  What is represented by  ΔT\Delta T  ?

a)

heat, measured in calories

b)

mass, measured in grams

c)

specific heat, in calories/gram/degree C

d)

temperature change in degree C

3.

The equation for heat transfer is  ΔQ = m×c×ΔT\Delta Q\ =\ m\times c\times\Delta T  What is represented by  mm  ?

a)

heat, measured in calories

b)

mass, measured in grams

c)

specific heat, in calories/gram/degree C

d)

temperature change in degree C

4.

Something that has a high specific heat capacity is likely to:

a)

stay at close to a constant temperature

b)

heat up easily and stay hot

c)

cool down easily and stay cold

d)

heat up and cool down easily

5.

The equation for heat transfer is  ΔQ = m×c×ΔT\Delta Q\ =\ m\times c\times\Delta T  Using this equation, figure out how much heat is required to warm up 2000 g of water from 20 degree C to 100 degrees C. Conveniently, the specific heat capacity of water is 1 cal/gram/degree C

a)

40,000 cal

b)

160,000 cal

c)

20,000 cal

d)

80,000 cal

6.

The equation for heat transfer is  ΔQ = m×c×ΔT\Delta Q\ =\ m\times c\times\Delta T  Using this equation, figure out how much heat is released when 100 grams of olive oil cool by 40 degrees C. The specific heat capacity of olive oil is c = 0.5 calories/gram/degree C.

a)

40 cal

b)

100 cal

c)

1000 cal

d)

2000 cal

7.
The study of heat released or absorbed by chemical reactions is called
a)
thermodynamics
b)
thermochemistry
c)
enthalphy
d)
entropy
8.
The S.I. unit for energy is
a)
calorie
b)
Kelvin
c)
grams
d)
joules
9.
The part of the world that we study in a chemical reaction is called the 
a)
universe
b)
surroundings
c)
system
d)
ecosystem
10.
A lizard uses the sun's rays to increase his body temperature. What type of energy transfer is occuring?
a)
Conduction
b)
Convection
c)
Condensation
d)
Radiation
11.
Heat always flows from _____ to ________
a)
cold to hot
b)
hot to cold
c)
top to bottom
d)
bottom to top
12.
The measure of heat flow into or out of a system due to physical or chemical processes is called
a)
calorimetry
b)
temperature
c)
energy
d)
specific heat
13.
Burning your hand on a hot dish from the oven exhibits what type of heat transfer
a)
conduction
b)
convection
c)
radiation
d)
thermochemistry
14.
How much energy is released when 2.5 Moles of gas condenses into water at the boiling point? 
 
Energy = (mole)(heat of vaporization) 
Hv = 40.79 KJ/mol
a)
-102 KJ
b)
15 KJ
c)
102 KJ
d)
-15 KJ
15.
Energy due to position or composition is _______energy. (stored)
a)
potential
b)
rapid
c)
kinetic
d)
heat
16.
The energy of motion is __________energy.
a)
potential
b)
rapid
c)
kinetic
d)
heat
17.
Using a hot plate in the chemistry lab to heat a beaker of water is an example of what type of heat transfer?
a)
conduction
b)
convection
c)
radiation
d)
thermochemistry
18.
In San Antonio, most air vents in homes are on the ceiling because this promotes cooler air circulating more efficiently in a warmer climate. AC systems are an example of what type of heat transfer?
a)
conduction
b)
convection
c)
radiation
d)
thermochemistry
19.

Kinetic molecular theory means-

a)

A molecule is always at rest

b)

A molecule is always in motion unless it is a solid

c)

A molecule is always in motion unless if reaches absolute zero

d)

Molecules do not move

20.

Which state of matter is the least dense?

a)

Solid

b)

Liquid

c)

Gas

d)

All are the same

21.

If all of these states of matter were poured in, which would settle from 0-50 in the graduated cylinder?

a)

Warm Gas

b)

Warm Liquid

c)

Warm Solid

d)

Cool Gas

e)

Cool Liquid

22.

Heat will always transfer from-

a)

Hot to Cold

b)

Cold to Hot

c)

High density to Low density

d)

Low energy to High energy

23.

Heat transfer by an egg on a frying pan is-

a)

Conduction

b)

Convection

c)

Radiation

24.

When it is hot your blood vessels _______ causing _______ heat to transfer to the skin

a)

Dilate; Less

b)

Dilate; More

c)

Constrict; Less

d)

Constrict; More

25.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
26.
Is the amount of energy that it takes to raise the temperature of 1 gram of a substance by 1 degree
a)
thermochemistry 
b)
heat 
c)
specific heat 
d)
chemical reaction
27.
If you rearrange the equation Q=mcT.  What does C equal?
a)
QmT
b)
Q/mT
c)
Qm/T
d)
Q X mT
28.
Process in which energy is released from the system 
a)
endothermic 
b)
exothermic
29.
Freezing water to make ice 
a)
Endothermic
b)
Exothermic 
30.
breaking a bond 
a)
endothermic 
b)
exothermic 
31.
In an exothermic reaction:
a)
ΔH is positive because energy is gained
b)
ΔH is negative because energy is gained
c)
ΔH is positive because energy is lost
d)
ΔH is negative because energy is lost
32.
forming a bond 
a)
endothermic 
b)
exothermic 
33.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
34.

Refer the the following question:

2N2 + 3H2 --> 2NH3 + 46 kJ

How much energy would be produced if only 1 mol of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

35.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
36.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
37.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
38.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
39.
What is a Chemical Reaction?
a)
When two liquids hit each other
b)
When a liquid has foam
c)
When two substances mix and produce new products
d)
When a reaction forms with soda and candy
40.
What is true of this reaction?
a)
Equal amounts of energy were released and absorbed
b)
The reaction released more energy than it absorbed
c)
The reaction absorbed more energy than it released
41.

What is the potential energy of the products? The energy readings are top 103, middle 45 and bottom 10

a)

10 kJ

b)

45 kJ

c)

103 kJ

d)

58 kJ

42.

What kind of reaction is this? The energy readings are top 103, middle 45 and bottom 10

a)

Endothermic

b)

Exothermic

c)

Cannot be determined

43.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
44.
Gases have...
a)
A definite shape and volume
b)
A definite shape but no definite volume
c)
No definite shape but a definite volume
d)
No definite shape or volume
45.
What is the correct temperature on the Kelvin scale equal to 30oC?
a)
303K
b)
243K
c)
313K
d)
253K
46.

If the temperature in a tank rises 15.6oC, how many Kelvin will it rise?

a)

25.6K

b)

288.6K

c)

273K

d)

15.6K

47.

Adding heat to a non-flexible container of gas will cause

a)

the molecules to slow down and hit the sides less often. The pressure will decrease.

b)

the temperature to increase and molecules to speed up. The pressure will not be affected.

c)

the molecules to speed up and hit the sides more often. The pressure will increase.

48.

The saturation temperature of water

a)

is 99.6oC

b)

is the constant temperature during evaporation

c)

is higher for saturated steam than for wet steam

d)

all of the above

49.

The density of steam is

a)

dependent on mass

b)

1000 kg/m3

c)

dependent on pressure and temperature

d)

calculated from pV=mRT

50.

The enthalpy needed to evaporate 1 kg of water at 2 bar is

a)

2202 kJ

b)

2707 kJ/kg

c)

2202 kJ/kg

d)

2530 kJ

51.

Wet steam has enthalpy

a)

higher than saturated water

b)

lower than dry steam

c)

dependent on dryness fraction

d)

all of the above

52.

Superheated steam has internal energy

a)

higher than wet steam

b)

decreasing with increasing temperature

c)

increasing with increasing pressure

d)

all of the above

53.

Steam at 1 bar and 110oC is

a)

saturated steam

b)

wet steam

c)

superheated steam

d)

there is not enough data to judge

54.

If saturated water and dry steam enthalpy at certain conditions is 1185 and 2790 kJ/kg respectively, then 50% wet steam enthalpy is:

a)

1205 kJ/kg

b)

802.5 kJ/kg

c)

1988 kJ/kg

d)

3125 kJ/kg

55.

Superheated steam from a boiler is known to have enthalpy of 3070x103 J/kg at 300oC, what is its pressure?

a)

30 bar

b)

3 MPa

c)

not enough data are given

d)

300 kPa

56.
Rank the following samples from greatest kinetic energy of the molecules to least kinetic energy of the molecules:
a)
A > B > C > D
b)
B > A > C > D
c)
B > A > D > C
d)
D > C > B > A
57.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
58.
When applying the first law of thermodynamics to a system, when is heat a positive quantity?
a)
when the system does work
b)
when the system has work done on it
c)
when the system absorbs heat
d)
when the system loses heat
e)
when no work is done either on the system or by the system
59.
The product of the pressure and volume of a system  has the same SI units as which one of the following choices?
a)
force
b)
work
c)
acceleration
d)
momentum
e)
impulse
60.

When an ideal gas expands at constant pressure, the change in the internal energy must be positive.

a)

True

b)

False

61.

A gas is heated by supplying it with 250 kJ of

energy; at the same time, it is compressed

so that 500 kJ of work is done on the gas.

Calculate the change in the internal energy of

the gas.

a)

250 kJ

b)

750 kJ

c)

-250 kJ

d)

500 kJ

62.

If an ideal gas is compressed isothermally, which of

the following statements is true?

a)

Energy is transferred to the gas by heat.

b)

No work is done on the gas.

c)

The temperature of the gas increases.

d)

The internal energy of the gas remains constant.

e)

None of those statements is true

63.
A Thermodynamic process is said to be Isovolumetric. This means that...
a)
∆U = 0
b)
Q = 0
c)
W = 0
d)
none of these
64.

(a)   energy is caused by the motion of particles.

65.

(a)   energy is the energy stored in the bonds of molecules.

66.

Which of the examples below shows thermal energy?

a)

Iron rusting

b)

Electricity going through a wire

c)

Rubbing hands together

d)

Water separated into hydrogen and oxygen gas

67.

Which of the examples below shows chemical energy?

a)

Baking a cake

b)

Rubbing hands together

c)

liquid water turning into ice

d)

Sugar being broken into ATP through respiration

68.

What type of system is shown?

a)

Open

b)

Closed

c)

Isolated

69.

Check all that apply


In an exothermic reaction the.....

a)

system gains energy

b)

system loses energy

c)

surrounding gains energy

d)

surrounding loses energy

70.

What type of process is this?

a)

Endothermic

b)

Exothermic

71.

What type of system does this show?

a)

Open system

b)

Closed system

c)

Isolated system

72.

Check all that apply


In an endothermic reaction the.....

a)

system gains energy

b)

system loses energy

c)

surrounding gains energy

d)

surrounding loses energy

73.

The law of conservation of energy describes how the amount of total energy can change in a closed system. Which of these statements correctly describes this law?

a)

The amount of kinetic energy in a system is a constant value.

b)

Energy can be converted from one form into another, but it cannot be created or destroyed.

c)

An object can have potential energy or kinetic energy, but not both at the same time.

d)

The amount of energy created when an object moves is equal to the energy destroyed when it stops moving.

74.

How is temperature related to heat?

a)

Temperature is a measure of the heat of an object.

b)

Heat causes a change in the temperature of an object.

c)

Raising the temperature causes the heat of an object to increase.

d)

Temperature and heat are two different ways to measure the same thing.

75.

Zara is warming a pot of soup on the stove. How is the motion of the particles in the soup different after the temperature of the soup increases?

a)

They move faster on average.

b)

They have less average energy.

c)

They move less freely.

d)

They vibrate and are close together

76.

Sonia notices that the temperature in the science lab is much colder than the temperature in her history classroom. Which of the following is true?

a)

The air molecules in the science lab are moving faster than those in the history classroom.

b)

The air molecules in the science lab are moving slower than those in the history classroom

c)

The air molecules in the science lab are moving at the same speed as those in the history classroom.

d)

The air molecules in the science lab are not moving while those in the history classroom are moving

77.

In what type of reaction do the products of the reaction always possess more potential energy than the reactants?

a)

redox

b)

exothermic

c)

spontaneous

d)

endothermic

78.

Which phase change is exothermic?

a)

H 2O( l) → H 2O( s)

b)

H 2O( l) → H 2O( s)

c)

H 2O( l) → H 2O( g)

d)

H 2O( s) → H 2O( g)

79.

How many joules of heat are required to raise the temperature of 20.0 grams of water from 30.0°C to 40.0°C?

a)

42 kj

b)

84 kj

c)

420 kj

d)

840kj

80.

The temperature of 50.0 grams of water was raised to 50.0°C by the addition of 4200 joules of heat energy. What was the initial temperature of the water?

a)

10.0°C

b)

20.0°C

c)

30.0°C

d)

60.0°C

81.

The temperature of a sample of water changes from 10°C to 20°C when the water absorbs 100 calories of heat. What is the mass of the sample?

a)

1 g

b)

10 g

c)

100 g

d)

1000 g

82.
The total energy of a system equals 
a)
its heat and temperature
b)
its work and temperature
c)
its heat and work
d)
its heat
83.

The first law of thermodynamics is a restatement of the

a)

Zeroth law of thermodynamics

b)

law of heat addition

c)

principle of entropy

d)

conservation of energy

84.

Which best describes ENTROPY?

a)

Useful heat energy needed to drive an engine

b)

Heat that can be stored to be used at a later date

c)

Degree of disorder of a state

d)

A state of order in a physical system

85.

Which statement is true about the ENTROPY?

a)

Entropy refers to disorder, the unusable portion that escapes from a system

b)

Entropy refers to the balance of temperature among two or more systems

c)

Entropy refers to the average kinetic energy of the molecules

d)

Entropy refers to the inability to destroy or create energy

86.

True or False? The First Law of Thermodynamics states that the total energy output is equal to the total amount of energy supplied.

a)

True

b)

False

87.

A system is in thermodynamic equilibrium

a)

if temperature and pressure at all points are same

b)

if temperature and pressure at all points are not same

c)

if temperature at all points are same

d)

if pressure at all points are same

88.

In an open thermodynamic system,

a)

heat can be transferred

b)

work can be done

c)

mass can be transferred

d)

all of the above

e)

none of the above

89.

When two bodies are in thermal equilibrium with a third body, they are also in thermal equilibrium with each other. This statement is called

a)

Zeroth law of thermodynamics

b)

First law of thermodynamics

c)

Second law of thermodynamics

d)

Kelvin Planck’s law

90.

The value of one bar (in SI units) is equal to

a)

100 N/m2

b)

1000 N/m2

c)

1 × 104 N/m2

d)

1 × 105 N/m2

e)

1 × 106 N/m2

91.
The _____ Law of Thermodynamics says that heat always flows from an object with a higher temperature to an object of lower temperature naturally
a)
Zeroth
b)
First
c)
Second
d)
Third
92.
Which law of thermodynamics states that absolute zero cannot be reached?
a)
1st
b)
2nd
c)
3rd
d)
Zeroth
93.

A system comprising a single phase is called a

a)

(a) closed system

b)

(b) open system

c)

(c) isolated system

d)

(d) homogeneous system

e)

(e) heterogeneous system.

94.

In an irreversible process, there is a

a)

(a) loss of heat

b)

(b) no loss of heat

c)

(c) gain of heat

d)

(d) no gain of heat.

95.

The unit of energy in SI units is

(J)

a)

(a) Joule (J)

b)

(b) Joule metre (Jm)

c)

(c) Watt (W)

d)

(d) Joule/metre (J/m).

96.

Which of the following is correct ?

a)

(a) Absolute pressure = gauge pressure + atmospheric pressure

b)

(b) Gauge pressure = absolute pressure + atmospheric pressure

c)

(c) Atmospheric pressure = absolute pressure + gauge pressure

d)

(d) Absolute pressure = gauge pressure – atmospheric pressure

97.

The value of one bar (in SI units) is equal to

a)

(a) 100 N/m2

b)

(b) 1000 N/m2

c)

(c) 1 × 104 N/m2

d)

(d) 1 × 105 N/m2

e)

(e) 1 × 106 N/m2.

98.

In an extensive property of a thermodynamic system

a)

(a) extensive heat is transferred

b)

(b) extensive work is done

c)

(c) extensive energy is utilised

d)

(d) all of the above

e)

(e) none of the above.

99.

Which of the following is an intensive property of a thermodynamic system ?

a)

(a) Volume

b)

(b) Temperature

c)

(c) Mass

d)

(d) Energy.

100.

Which of the following is the extensive property of a thermodynamic system ?

a)

(a) Pressure

b)

(b) Volume

c)

(c) Temperature

d)

(d) Density.

101.

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

each other. This statement is called

a)

(a) Zeroth law of thermodyamics

b)

(b) First law of thermodynamics

c)

(c) Second law of thermodynamics

d)

(d) Kelvin Planck’s law.

102.

Absolute zero temperature is taken as

a)

(a) – 273°C

b)

(b) 273°C

c)

(c) 237°C

d)

(d) – 373°C.

103.

The force exerted by the system on unit area of boundaries is called

a)

Pressure

b)

Volume

c)

density

d)

viscosity

104.

A system is in thermodynamic equilibrium

a)

if temperature and pressure at all points are same

b)

if temperature and pressure at all points are not same

c)

if temperature at all points are same

d)

if pressure at all points are same

105.

A pure substance is one that has even though there

is a change of phase

a)

a homogeneous

b)

a homogeneous and invariable chemical composition

c)

invariable chemical composition

d)

none of the above

106.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
107.
A(n) _____________ is a device for measuring temperature.
a)
thermometer
b)
barometer
c)
anemometer
d)
psychrometer 
108.
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
109.
Heat transfer by conduction occurs when...
a)
particles bump into each other
b)
large numbers of atoms move from place to place
c)
atoms give off heat in the form of electromagnetic waves
d)
electromagnetic waves travel from place to place through a vacuum
110.
Heat transfer by convection occurs when...
a)
electrons bump into other electrons
b)
large numbers of atoms move from place to place
c)
atoms give off heat in the form of electromagnetic waves
d)
electromagnetic waves travel from place to place through a vacuum
111.
The second  law of thermodynamics states that entropy of a system  tends to ______________. 
a)
increase
b)
decrease
c)
stay constant
d)
fluctuate wildly
112.
The temperature of a glass of cold water will eventually...
a)
Match the temperature of the surrounding environment.
b)
Always be colder than the surrounding environment.
c)
Become warmer than the surrounding environment.
d)
Never change temperature.
113.
Which law of thermodynamics states that absolute zero cannot be reached?
a)
1st
b)
2nd
c)
3rd
114.
The first law of thermodynamics states that energy is
a)
created
b)
destroyed
c)
conserved
d)
created and destroyed
115.

which of the following laws is applicable for the behaviour of perfect gas...

a)

Boyle's law

b)

Charle's Law

c)

Gas Lussac law

d)

All of the above

116.

A thermodynamic system where no exchange of heat takes place between system and surrounding is...

a)

Isothermal process

b)

Adiabatic process

c)

Isobaric process

d)

Isochoric process

117.

dQ=dU+dW refers to which law of Thermodynamic?

(a)  

118.
The handle of a metal spoon warms up when it is placed in a hot bowl of soup because of
a)
Convection
b)
Conduction
c)
Radiation
d)
insulation.
119.
The first law of thermodynamics states that the change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and
a)
mass
b)
work done
c)
force
d)
pressure
120.
The first law of thermodynamics is a restatement of the
a)
Zeroth law of thermodynamics
b)
law of heat addition
c)
principle of entropy
d)
conservation of energy
121.

which of the following laws is applicable for the behaviour of perfect gas...

a)

Boyle's law

b)

Charle's Law

c)

Gas Lussac law

d)

All of the above

122.

A thermodynamic system where no exchange of heat takes place between system and surrounding is...

a)

Isothermal process

b)

Adiabatic process

c)

Isobaric process

d)

Isochoric process

123.
What does the "U" stand for the formula ∆U = Q + W
a)
Heat
b)
Temperature
c)
Work
d)
Internal energy
124.

Heating a closed, steel container is an example of an

a)

Adiabatic process

b)

Isovolumetric process

c)

Isothermal process

d)

Isobaric process

125.

Which of the following equations is the equation for calculating the work done by a gas in a piston?

a)

W=Fd

b)

W=PΔV

c)

ΔV=Ad

d)

A=πr2

126.

Symbol that indicates that energy is released.

a)

U

b)

Q

c)

-Q

d)

W

127.

In an adiabatic process, what equals zero?

a)

Q

b)

W

c)

ΔU

d)

T

128.

The PV diagram for an adiabatic process looks similar to the PV diagram for...

a)

... Isochoric process

b)

...Isothermal process

c)

... Isobaric process

d)

It does not look similar to any of these charts

129.

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 of the gas?

a)

800 J

b)

1600 J

c)

-800 J

d)

-1600 J

130.

During an adiabatic process, a sample of gas does 400 J of work on the environment. What change occurs with the internal energy of the gas?

a)

The internal energy increases by 400 J.

b)

The internal energy doesn't change.

c)

The internal energy decreases by 400 J.

d)

There is not enough information if we don't know how much heat was added or removed.

131.

Process B on the PV diagram is an ______________ process.

a)

adiabatic

b)

isobaric

c)

isochoric

d)

isothermal

132.

If the temperature of a gas increases and there is negative work done on the gas, then...

a)

there must be heat added to the gas

b)

the gas must be giving off heat to the environment.

c)

this is an adiabatic process.

d)

there must be less heat added than the work done on the gas.

133.

The average kinetic energy of the atoms or molecules in a substance is directly related to

a)

heat

b)

specific heat capacity

c)

temperature

d)

Brownian Motion

134.

What is heat?

a)

the amount of thermal energy in an object

b)

an object's internal kinetic energy

c)

the transfer of thermal energy from one object to another

d)

the amount of energy needed to raise the temp of an object

135.

During process D, from state 4 to state 1, the ideal gas...

a)

is increasing temperature.

b)

is doing work on the environment.

c)

is decreasing pressure.

d)

is decreasing temperature.

136.

Specific Heat is..

a)

the temperature initial minus temperature final

b)

the amount of heat/energy required to raise 1 gram of a substance by 1°C (or K) aka "C"

c)

the temperature final minus temperature initial

d)

the item in a system with given weight in grams

137.

A system is in thermodynamic equilibrium

a)

if temperature and pressure at all points are same

b)

if temperature and pressure at all points are not same

c)

if temperature at all points are same

d)

if pressure at all points are same

138.

Energy cannot be created or destroyed.

a)

0th law

b)

1st law

c)

2nd law

d)

3rd law

139.

Which is an example of the 0th law?

a)

0 Kelvin

b)

Chaos cannot decrease

c)

A=B=C

d)

U = W - q

140.
What is "Entropy"?
a)
The tendency of objects to warm up
b)
The tendency of energy to spread out
c)
The tendency of energy to make heat
d)
The tendency of objects to do work
141.

The 2nd Law of Thermodynamics tells us...

a)

Heat flows from cold to hot.

b)

Heat flows randomly, it's a 50/50 coin flip

c)

Heat doesn't flow, temperature flows.

d)

Heat flows from hot to cold.

142.
What is the name of a device that converts thermal energy into work?
a)
Heating system
b)
Heat engine
c)
Entropy
d)
Power
143.

In the polytropic process pvn = Constant if n = 1 the process is termed as

a)

A.Constant volume

b)

B.Constant pressure

c)

C.Constant temperature

d)

D.Adiabatic

e)

E.Isothermal

144.

A law which is applicable only to ideal vapours and liquids, that equates the equilibrium partial pressures of a solution component in the coexisting phases, is known as

a)

A.Henry's law

b)

B.Roult's law

c)

C.Joule's law

d)

D.Maxwell's equation

e)

E.Fick's law

145.

The molecular volume of any perfect gas at 600 x 103 N/m3 and 27?C will be

a)

A.2.085 m3/kg mol

b)

B.4.17 m3/kg mol

c)

C.41.7 m3/kg mol

d)

D.85.3 m3/kg mol

e)

E.47.7 m3/kg mol

146.

An open system

a)

A.Is a specified region where transfers of energy and/or mass take place

b)

B.Is a region of constant mass and only energy is allowed to cross the boundaries

c)

C.Cannot transfer either energy or mass to or from the surroundings

d)

D.Has a mass transfer across its boundaries, and the mass within the system is not necessarily constant

e)

E.None of the above

147.

A system consisting of more than one phase is known as

a)

A.Open system

b)

B.Closed system

c)

C.Isolated system

d)

D.Non-uniform system

e)

E.Heterogeneous system

148.

Whenever a system undergoes either a change in state or an energy or mass transfer at a steady state, it is said to undergo

a)

A.Achange of state

b)

B.A process

c)

C.A steady state transfer

d)

D.An equilibrium

e)

E.A thermodynamic change

149.

The processes or systems that do not involve heat are called

a)

A.Isothermal processes

b)

B.Equilibrium processes

c)

C.Thermal processes

d)

D.Steady processess

e)

E.Adiabatic processe

150.

Which of the following are macroscopic forms of energy:

(a). Kinetic Energy

(b) Potential Energy

(c) Rotational KE of molecules

(d) Chemical energy of molecules

a)

(a) & (c)

b)

(b) & (d)

c)

(a) & (b)

d)

(a) & (d)

151.

Which of the following are microscopic forms of energy:

(a). Kinetic Energy

(b) Potential Energy

(c) Rotational KE of molecules

(d) Chemical energy of molecules

a)

(a) & (b)

b)

(a) & (c)

c)

(b) & (d)

d)

(c) & (d)

152.

A closed system, with no change in KE and PE, is called

a)

Control Volume

b)

Stationary System

c)

Flow System

d)

Isolated system

153.

For a flow process in a control volume, the mass flow rate of the fluid is given by

a)

ρAcVave\rho A_cV_{ave}

b)

ρAcVave\frac{\rho A_c}{V_{ave}}

c)

ρVaveAc\frac{\rho V_{ave}}{A_c}

d)

AcVaveρ\frac{A_cV_{ave}}{\rho}

154.

For a statinary system

a)

ΔE = ΔU\Delta E\ =\ \Delta U

b)

ΔE = ΔPE\Delta E\ =\ \Delta PE

c)

ΔE = ΔKE\Delta E\ =\ \Delta KE

d)

ΔE = ΔPE+ΔKE\Delta E\ =\ \Delta PE+\Delta KE

155.

Which of the following is not the equation for adiabatic process

a)


TVγ−1 = CTV^{\gamma-1}\ =\ C

b)

PVγ PV^{\gamma\ } = Constant

c)

PV = Constant

d)

P1−γTγ= C.P^{1-\gamma}T^{\gamma}=\ C. = constant.

156.

Correct Meyer's relation

a)

Cp-Cv = R

b)

Cv-Cp = R

c)

Cv+Cp = R

157.

First law of thermodynamics represents

a)

law of conservation of energy

b)

law of entropy

c)

law of heat conservation

d)

thermal equilibrium

158.
Which state of H2O  has the greatest entropy?
a)
Ice
b)
Water
c)
Vapor
159.

How much work is done by 0.020 m3 of gas if its pressure increases by 2.0 x105 Pa and the volume remains constant?

a)

a. 0 J

b)

b. -4.0 x 103 J

c)

c. 4.0 x103 J

d)

d. 1.0 x107 J

160.

Which of the following are ways in which energy can be transferred to or from a substance?

a)

a. heat and internal energy

b)

b. work and internal energy

c)

c. heat and work

d)

d. heat and kinetic energy

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