Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

ARC > PHYSICAL CHEMISTRY > Flashcards

PHYSICAL CHEMISTRY Flashcards

1
Q

An ideal gas will only be considered in the
following operating parameters:

a. High Temperature, High Pressure
b. High Temperature, Low Pressure
c. Low Temperature, High Pressure
d. Low Temperature, Low Pressure

A

b. High Temperature, Low Pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Which of the following is false regarding absolute
zero?

a. All molecules will stop moving
b. Absolute zero can be achieved
c. Temperature is 0K
d. Temperature is 0R

A

b. Absolute zero can be achieved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

For a real gas, what causes the deviation from the
ideal pressure at a molecular level?

a. Energy is lost for each collision against
the sides of the container
b. Energy is lost due to the collision of
molecules with one another
c. Intermolecular forces of attraction of the
molecules with one another
d. Molecules randomly hit the sides of the
wall with less force than usual

A

c. Intermolecular forces of attraction of the
molecules with one another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

When gas molecules collide, they experience
_____ collision.

a. Perfectly elastic
b. Imperfect elastic
c. Perfectly inelastic
d. Imperfect inelastic

A

a. Perfectly elastic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Which of the following is false with KMT?

a. Gas molecules move in random motion
b. Due to collision of gas molecules with
each other, some kinetic energy is lost
c. The temperature of the whole system
does not change with time
d. The size of the molecules are negligible

A

b. Due to collision of gas molecules with
each other, some kinetic energy is lost

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

The internal energy of an ideal gas depends on:

a. Volume
b. Absolute temperature
c. Pressure
d. Number of moles

A

b. Absolute temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

The state of an ideal gas is changed in a closed
path 1→2→3→4→1. Which of the following is
true about the work done on the gas?

| P  |    2  \_\_\_\_\_\_\_\_\_\_\_\_\_ 3
|       |                    |
|    1 |\_\_\_\_\_\_\_\_\_\_\_\_|4
|
|\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_
                  V

a. W12>0, W23=0, W34<0, W41=0
b. W12<0, W23=0, W34=0, W41>0
c. W12=0, W23>0, W34=0, W41<0
d. W12=0, W23<0, W34=0, W41>0

A

d. W12=0, W23<0, W34=0, W41>0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Which of the following is a characteristic of an
adiabatic process?

a. ΔU=0
b. W=0
c. Q=0
d. ΔV=0

A

c. Q=0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

A sample of an ideal gas has an internal energy of
U and is then compressed to ½ of its original
volume while the temperature stays the same.
What is the new internal energy of the ideal gas
in terms of U?

a. U
b. U/2
c. U/4
d. 2U

A

a. U

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Which of the following is not conserved in any
process?

a. Mass
b. Energy
c. Momentum
d. Entropy

A

d. Entropy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

An isentropic process is:

a. Isothermal and adiabatic
b. Reversible and isothermal
c. Reversible and adiabatic
d. Reversible and isochoric

A

c. Reversible and adiabatic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Increasing the temperature of the cold reservoir
_____ the Carnot efficiency.

a. Increases
b. Decreases
c. Does not change
d. NOTA

A

b. Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

If the entropy of a system decreases, the entropy
of its surroundings

a. Must always increase
b. Must always decrease
c. May increase or decrease
d. Not enough information to answer the
question

A

a. Must always increase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Which of the following is not true?

a. (
𝜕𝐺
/𝜕𝑃)
𝑇
= 𝑉
b. (
𝜕𝐻
/𝜕𝑃)
𝑇
= 𝑉
c. (
𝜕𝐺
/𝜕𝑇)
𝑃
= −𝑆
d. (
𝜕𝐻
/𝜕𝑉)
𝑇
= −𝑆

A

d. (
𝜕𝐻
/𝜕𝑉)
𝑇
= −𝑆

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

The amount of heat absorbed when CO2 gas
reacts with a solid CaO to form solid CaCO3 is
measured in a bomb calorimeter. The data
obtained give a direct measure of:

a. ΔU
b. VΔP
c. ΔH
d. Cp

A

a. ΔU

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Heat required to raise the temperature of 1lbm of
water by 1˚F.

a. Calorie
b. BTU
c. Specific heat
d. Heat capacity

A

b. BTU

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Which of the following statements is/are true?
1. The criterion of equilibrium at constant
temperature and pressure is dG=0.
2. For a reversible process, dS=dQ/T.

a. 1 only
b. Both 1 and 2
c. 2 only
d. None of the above

A

b. Both 1 and 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

The general statement of the Third Law of
Thermodynamics is attributed to:

a. Nikolaus Otto
b. Jacobus Clapeyron
c. William Clausius
d. Walther Nernst

A

d. Walther Nernst

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

The equilibrium intensive state of a system is
described by specifying the temperature,
pressure, and:

a. Mole fractions
b. Number of moles
c. Volume
d. Chemical potential

A

a. Mole fractions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

The fugacity of a real gas is equal to:

a. The pressure of an ideal gas which has
the same chemical potential as the real
gas
b. The pressure of a real gas which has the
same chemical potential as the ideal gas
c. The chemical potential of an ideal gas
which has the same pressure as the real
gas
d. The chemical potential of a real gas
which has the same pressure as the ideal
gas

A

a. The pressure of an ideal gas which has
the same chemical potential as the real
gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

An adiabatic process is one in which the system
under investigation is thermally isolated so that
there is no exchange of heat with the surroundings. Thus, the work done on a closed
system in an adiabatic process is _____.

a. Equal to zero
b. Not equal to the exchange of heat with
surroundings
c. Equal to the increase in internal energy of
the system
d. Not equal to the increase in internal
energy of the system

A

c. Equal to the increase in internal energy of
the system

22
Q

If enthalpy is defined as present in a constant
pressure process change of state, using the
relationship of ΔH=ΔU+ΔPV, where H is
enthalpy, U is the energy change in the system
and PV represents pressure and volume states,
determine the ΔU and ΔH of 1kg of water when
vaporized at constant temperature of 100˚C and
constant pressure of 101.35kPa. The specific
volumes of liquid and vapor water are 0.001041
and 1.67m3
/kg. An amount of 2257kJ of heat is
added to the water.

a. ΔU=2087kJ; ΔH=2257kJ
b. ΔU=2378kJ; ΔH=2221kJ
c. ΔU=2226kJ, ΔH=2378kJ
d. None of these

A

a. ΔU=2087kJ; ΔH=2257kJ

23
Q

A certain gas confined in a cylinder by a piston,
where the initial pressure in the system is 7 bar
and the volume is 0.11 cubic meter. The piston is
held in place by latches and the apparatus is in
vacuum. Determine the change in energy when
the latches are removed suddenly and the gas
expands to double its initial volume and the piston
strikes the latches at the end of the process.

a. 11.54kJ
b. 0.77kJ
c. 0.59kJ
d. No change

A

d. No change

24
Q

Define entropy.

a. Entropy is a function of the state of the
system and determines whether a
physical change or chemical reaction can
occur simultaneously in a closed system
b. Entropy is the opposite of enthalpy
c. Entropy determines the time required for
a reaction to proceed and complete
d. All of these

A

d. All of these

25
Q

Determine whether the changes in entropy (ΔS)
and enthalpy (ΔH) are positive, negative, or near
zero.
1. Ethyl alcohol evaporating from glass
container
2. A diatomic molecule dissociates into
atoms
3. Charcoal is burned to form CO2 and
water

a. 1. ΔH>0, ΔS>0; 2. ΔH>0, ΔS>0; 3.
ΔH>0, ΔS>0
b. 1. ΔH<0, ΔS<0; 2. ΔH>0, ΔS<0; 3.
ΔH>0, ΔS<0
c. 1. ΔH>0, ΔS<0; 2. ΔH<0, ΔS>0; 3.
ΔH>0, ΔS>0
d. 1. ΔH<0, ΔS>0; 2. ΔH<0, ΔS<0; 3.
ΔH<0, ΔS<0

A

a. 1. ΔH>0, ΔS>0; 2. ΔH>0, ΔS>0; 3.
ΔH>0, ΔS>0

26
Q

Choose the process that occurs with a decrease in
entropy.

a. Freezing of water
b. Boiling of water
c. Dissolving salt in water
d. Sublimation of dry ice

A

a. Freezing of water

27
Q

A vessel of volume 22.4 dm3
contains 2
mol H2 and 1 mol N2 at 273.15 K. What
is the total pressure inside the vessel?
Assume ideal gas.

a. 1 atm
b. 2 atm
c. 3 atm
d. 4 atm

A

c. 3 atm

28
Q

In an industrial process, nitrogen is
heated to 500 K at a constant volume of
1 m3
. The gas enters the container at 300
K and 100 atm. Use the Van der Waal’s
equation to determine the approximate
pressure of the gas at its working
temperature of 500 K. For nitrogen, a =
1.352 dm6
-atm / mol2
,
b = 0.0387
dm3
/mol.

a. 120 atm
b. 140 atm
c. 160 atm
d. 180 atm

A

d. 180 atm

29
Q

A perfect gas undergoes isothermal
compression, which reduces its volume
by 1.8 dm3
. The final pressure and
volume of the gas are 1.97 bar and 2.14
dm3
, respectively. Calculate the original
pressure of the gas.

a. 10.5 bar
b. 1.07 bar
c. 750 torr
d. 850 torr

A

b. 1.07 bar

30
Q

At 100 ˚C and 1.6 kPa, the mass density
of phosphorus vapor is 0.06388 kg/m3
.
What is the molecular formula of
phosphorus under these conditions?

a. P
b. P2
c. P3
d. P4

A

d. P4

31
Q

A 1 dm3 glass bulb contains 1x1023 H2
molecules. If the pressure exerted by the
gas is 100 kPa, assuming ideal gas,
determine the temperature of the gas.

a. 56.54 K
b. 72.43 K
c. 103.64 K
d. 159.64 K

A

b. 72.43 K

32
Q

5000 J of heat are added to 2 mol of an
ideal monoatomic gas, initially at a
temperature of 500 K, while the gas
performs 7500 J of work. What is the
final temperature of the gas?

a. 200 K
b. 300 K
c. 400 K
d. 500 K

A

c. 400 K

33
Q

What is the final temperature of a sample
of argon of mass 12 g that is expanded
reversibly and adiabatically from 1 dm3
and 273.15 K to 3 dm3
?

a. 122 K
b. 131 K
c. 145 K
d. 159 K

A

b. 131 K

34
Q

A sample of 4.5 g of methane occupies 12.7 dm3
at 310 K.

Calculate the work done when a gas
expands isothermally against a constant
external pressure of 200 torr until its
volume has increased by 3.3 dm3
a. -79 J
b. -150 J
c. -126 J
d. -88 J

Calculate the work that would be done if
the same expansion occurred reversibly
and isothermally.
a. -150 J
b. -167 J
c. -103 J
d. -120 J

A

d. -88 J

b. -167 J

35
Q

(Nov. 2019 PBE) Applying the combined
gas laws, determine the volume of 1 mol
of Ne(g) in a flask at the temperature of 25
˚C and a pressure of 1 atm.

a. 12.2 L
b. 18.6 L
c. 32.21 L
d. 24.51 L

A

d. 24.51 L

36
Q

(Nov. 2019 PBE) In the combustion of 25
g of methane gas, what is the volume of
oxygen required at 25 ˚C and 0.21 atm?

a. 411
b. 298
c. 363
d. 521

A

c. 363

37
Q

(Nov. 2019 PBE) Determine the volume
of carbon dioxide in cubic feet occupied
by 120 lb at a pressure of 1.5 atm.

a. 750
b. 490
c. 560
d. 680

A

a. 750

38
Q

(Nov. 2019 PBE) If 1 mol of an ideal gas
is kept at 0 ˚C, during an expansion from
3.0 to 10.0 L, examine and calculate how
much work is done as the gas during
expansion.

a. -2.2x10^4 J
b. -5.4x10^3 J
c. -7.8x10^4 J
d. -2.7x10^3 J

A

d. -2.7x10^3 J

39
Q

(Oct. 2021 PBE) In a gas mixture
containing 100 mg/L of H2S gas at 25 ˚C
and 1 atm, determine the partial pressure
exerted by the gas.

a. 0.071
b. 0.003
c. 0.101
d. 0.006

A

a. 0.071

40
Q

Which of the following does not have a zero
enthalpy of formation at 298.15K?

a. Li(g)
b. He(g)
c. Hg(l)
d. Br2(l)

A

a. Li(g)

41
Q

Calculate the enthalpy change of the
reaction (in kJ/mol).
CS2(l) + 3O2(g) → CO2(g) + 2SO2(g)

C(s) + O2(g) → CO2(g); ΔHF = -393.5
kJ/mol
S(s) + O2(g) → SO2(g); ΔHF = -296.8
kJ/mol
C(s) + 2S(s) → CS2(l); ΔHF = 87.9 kJ/mol

a. -900
b. -1100
c. -1300
d. -1500

A

b. -1100

42
Q

(Nov. 2019 PBE) Calculate the net and
the gross heats of combustion for
methane gas.

a. -491 kJ; -998 kJ/mol
b. -362 kJ; -731 kJ/mol
c. -891 kJ/mol; -802 kJ/mol
d. -598 kJ; -1120 kJ/mol

A

c. -891 kJ/mol; -802 kJ/mol

43
Q

(Nov. 2019 PBE) If 5 g of methane gas is
burned at constant pressure, determine
the heat released in kJ if the change in
entropy that accompanied the reaction is
-890 kJ.

a. -360.00 K
b. -250.01 K
c. -278.12 K
d. -192.00 K

A

c. -278.12 K

44
Q

(Oct. 2021) The standard molar enthalpy
change is -905 kJ for the oxidation of
ammonia, 4NH3(g) + 5O2 → 4NO(g) +
6H2O(g). Analyze and calculate the standard molar enthalpy of formation for
ammonia based on the following
standard enthalpies of formation:
HF[NO(g)] = +90 kJ/mol; and HF[H2O(g)] = -
240kJ/mol

a. -227 kJ/mol
b. -500 kJ/mol
c. -406 kJ/mol
d. -692 kJ/mol

A

a. -227 kJ/mol

45
Q

A block of iron weighing 3.6 kg at a temperature
of 807 ˚C was inserted into a container containing
1 L of water at a temperature of 30 ˚C isolated
from the environment. The cooling process of
iron happens in two steps, the first phase the water
is heated the boiling point and in the second stage
the water evaporates. The phase continues until
the temperature of the iron is equal to the
temperature of the water. The final temperature of
the water and the iron is 100 ˚C. The specific heat of solid iron is 0.45 J/g-K and the heat of
vaporization for water is 2259.23 J/g.

The energy given off by the iron block in
MJ is nearest to:
a. 1.1
b. 1.3
c. 0.7
d. 0.9

How much sensible heat was used by the
water to get to its boiling point in J?
a. 200,000
b. 300,000
c. 400,000
d. 500,000

The amount of water vaporized in grams
in this process is nearest to:
a. 200
b. 300
c. 400
d. 500

If the density of water at all temperatures
is 1 g/mL, The amount of water left in the
container in L is:
a. 0.5
b. 0.6
c. 0.7
d. 0.8

A

a. 1.1

b. 300,000

c. 400

b. 0.6

46
Q

A 2 kg open calorimeter at 100 ˚C has a heat capacity of 4 kJ/K. 100 g of ice at -10˚ C was
placed inside the calorimeter. If CP of ice = 0.5
cal/g-K and latent heat of fusion is 80 cal/g,

Calculate the final temperature in ˚C.
a. 78
b. 82
c. 86
d. 90

Calculate the entropy change of the
calorimeter in cal/K.
a. -184
b. -92
c. -46
d. -24

Calculate the entropy change of the ice in
cal/K.
a. 200
b. 100
c. 60
d. 40

Calculate the entropy change of the
universe in cal/K.
a. 12
b. 14
c. 16
d. 18

A

b. 82

c. -46

c. 60

a. 12

47
Q

Ethanol may be treated as an
incompressible fluid at an appreciable
pressure range. If the pressure is changed
from 1 bar to 3 bar at 350 K, what is the
change in the Gibbs free energy in J/g?
The density of ethanol at this temperature
is 800 kg/m3
.

a. 0.25
b. 2.5
c. 25
d. 250

A

a. 0.25

48
Q

What is the minimum work in BTU
required to produce 20 lb of ice from
water at 32 ˚F if the surrounding air is 85
˚F and the latent heat of fusion of ice is
143.4 BTU/lb?

a. 300
b. 310
c. 320
d. 330

A

b. 310

49
Q

It is the property of a fluid that is caused by
shearing effect of a fluid layer moving past
another layer.

a. Density
b. Viscosity
c. Flow
d. Compressibility

A

b. Viscosity

50
Q

A sphere of radius 5 mm and density of
1.1 g/cm3
falls at a constant velocity
through a liquid of density 1 g/cm3
and
viscosity of 1 cP. What is the velocity of
the falling sphere in m/s?

a. 1.36 m/s
b. 2.72 m/s
c. 5.45 m/s
d. 10.88 m/s

A

c. 5.45 m/s

51
Q

An Ostwald Viscometer is used to
measure the viscosity of a monoatomic
gas. The inlet and outlet pressures of the
gas are 1.1 atm and 1.08 atm. What is the
viscosity in μP of 100 mL of this gas
measured at 300 K if it took 5 s for the
gas to flow through a 0.5 m tube of 1 mm
diameter?

a. 0.5
b. 5
c. 50
d. 500

A

c. 50

52
Q

An Ostwald Viscometer is used to
measure the viscosity of a monoatomic
gas. The inlet and outlet pressures of the
gas are 1.1 atm and 1.08 atm. What is the
viscosity in μP of 100 mL of this gas
measured at 300 K if it took 5 s for the
gas to flow through a 0.5 m tube of 1 mm
diameter?

a. 0.5
b. 5
c. 50
d. 500

A

c. 50

ARC (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions