__Temperature &
Pressure Conversions__

I. Convert the following
units of pressure:

1.) 2.00 atm to mm Hg

2.) 115 kPa to atm

3.) 500. mm Hg to atm

4.) 3.5 x 10^{4} torr to mm Hg

5.) 1800. mm Hg to kPa

6.) 93,500 Pa to atm

7.) 950. torr
to atm

8.) 0.490 atm to kPa

II. Convert the following temperature readings:

1.) 35 ^{o}C to Kelvin

2.) 120 ^{o}C
to Kelvin

3.) -25 ^{o}C
to Kelvin

4.) -227 ^{o}C
to Kelvin

5.) standard temperature in
Kelvin and Celsius

6.) 298 K to ^{o}C

7.) 100. K to ^{o}C

8.) 5 Kelvin to ^{o}C

__Ideal Gas
Equation 1 __

1.) What is the pressure exerted by 2.0 moles of
an ideal gas when it occupies a volume of 12.0 L at

373 K?

2.) A flashbulb of volume 2.6 cm^{3}
contains O_{2} gas at a pressure of 2.3 atm
and a temperature of 26^{o}C.

How many moles of O_{2}
does the flashbulb contain? (Answer: 2.4 x 10^{-4}
moles)

3.) If 0.20 moles of helium occupies a
volume of 64.0 liters at a pressure of 0.15 atm, what
is the

temperature of the gas? (Answer:
580 K)

4.) What is the volume of 0.35 moles of
gas at 1.7 atm of pressure and a temperature of 100 K?

5.) What is the pressure of 1.5 moles of
an ideal gas at a temperature of 150 K and occupies a volume

of 20.0 liters? (Answer:
0.92 atm)

6.) How many moles of gas occupy 16.2
liters at a pressure of 1.05 atm and a temperature of
37^{o}C?

(Answer:
0.668 moles)

** Ideal
Gas Equation 2 **1. Calculate the
volume of exactly 1.00 mole of a gas at STP. (22.4
L)

2. How many moles of nitrogen are present in 17.8 liters at
27 ^{o}C and 1.3 atm
pressure? (0.94 moles)

3. What is the pressure of 2.3 moles of carbon dioxide at 235
K occupying 23.7 liters of space? (1.9
atm)

4. If there are 4.02 x 10^{23} molecules of N_{2}O
in a sample, how many moles are there? (0.668
moles)

5. Using your answer from # 6,
calculate the pressure of the gas if it occupies 27,025 cm^{3} of space

at 38.0 ^{o}C. (0.631
atm)

6. How many grams of ammonia gas (NH_{3}) are present
in 35.0 dm^{3} of space at 78.3 K and 0.853 atm

of pressure? (78.9
g)

7. What is the temperature of 34.2 grams of sulfur dioxide
occupying 30.0 liters of space and having

a pressure of 800.
torr? (720.
K)

8. What is the pressure (in mm Hg) of 79.4 grams of boron trifluoride with a volume of 20.0 L and

a temperature of 245 K? (889
mm Hg)

9. How many grams are in a sample of arsenic trifluoride
that has a volume of 17,600 mL and a

temperature of 92 ^{o}C and a pressure of 108,732 Pa? (83
g)

10. How many kilopascals of pressure are exerted by 23.8 liters of
oxygen with a mass of 175 grams

at a temperature of 58 ^{o}C? (632
kPa)

11. How many moles of argon are in 30.6 liters at 28 K and
658 mm Hg of pressure? (12
moles)

12. How many grams of argon are found in # 11? (480
g)

** Applications
of Ideal Gas Equation**1.) What pressure is exerted by
1.0 mole of an ideal gas contained in a 1.0 L vessel at 0.0

(Answer: 22 atm)

2.) What is the density of a sample of ammonia gas, NH_{3}, if
the pressure is 0.928 atm and the

temperature is 63.0 ^{o}C? (Answer:
0.572 g/L)

3.) Calculate the
molar mass of a gas if 4.5 L of the gas at 785 torr
and 23.5 ^{o}C has a mass of 13.5

grams. (Answer:
71 g/mole)

4.) 0.453 moles of a
gas confined to a 15.0 L container exerts a pressure of 1.24 atm on the walls of

the container. What is the
temperature of the gas (in ^{o}C)? (Answer: 227 ^{o}C)

5.) 5.4 grams of
carbon dioxide are confined to a 20.0 L container at a temperature of 32.5 ^{o}C. What

pressure does the gas exert? (Answer:
0.15 atm)

6.) 2.125 grams of a
gas in a 1.25 L container exert a pressure of 0.838 atm
at 40.0 ^{o}C. What is the

molar mass of the gas? (Answer:
52.1 g/mole)

7.) To what
temperature must 10.0 grams of ammonia gas (NH_{3}) have to be heated
in a 15.0 L

container in order for it to exert
a pressure of 3.50 atm? (Answer: 1090 K)

8.) 2.0 x 10^{-5}
grams of hydrogen gas at 155 ^{o}C exert a
pressure of 322.5 torr on the walls of a small

cylindrical tube. What is the
volume of the tube? (Answer:
8.3 x 10^{-4} L)

__Gas Law Problems __

1.) The gas pressure in an aerosol can is 1.5 atm at 25 ^{o}C. Assuming that the gas inside obeys the

ideal gas equation, what would the
pressure be if the can were heated to 450 ^{o}C?

2.) A pocket of gas is discovered in a deep
drilling operation. The gas has a
temperature of 480 ^{o}C

and is at a pressure of 12.8 atm. Assume ideal
behavior. What volume of the gas is
required to

provide 18.0 L at the surface at
1.00 atm and 22 ^{o}C?

3.) A
fixed quantity of gas is compressed at constant temperature from a volume of
368 mL to 108

mL. If the initial pressure was 5.22 atm, what is the final pressure?

4.) A
gas originally at 15 ^{o}C and having a
volume of 182 mL is reduced in volume to 82.0 mL while its

pressure is held constant. What is its final temperature?

5.) At
36 ^{o}C and 1.00 atm
pressure, a gas occupies a volume of 0.600 L.
How many liters will it

occupy at 0.0 ^{o}C
and 0.205 atm?

6.) What
is the temperature at which 9.87 x 10^{-2} moles occupies 164 mL at 0.645 atm?

7.) Chlorine
is widely used to purify municipal water supplies and to treat swimming pool
waters.

Suppose that the volume of a
particular sample of Cl_{2} is 6.18 L at 0.90 atm
and 33 ^{o}C.
What

volume will the Cl_{2 }occupy
at 107 ^{o}C and 0.75 atm?

8.)
A gas exerts a pressure of 1.5 atm at 27 ^{o}C. The
temperature is increased to 108 ^{o}C with no

volume change. What is the gas pressure at the higher
temperature?

Answers:
1.) 3.6 atm
2.) 3.59 L or 3.6
L 3.) 17.8 atm
4.) 130 K or 130. K

5.) 2.59 L or 2.6
L
6.) 13.1
K
7.) 9.2
L
8.) 1.9 atm

__GAS STOICHIOMETRY (standard
conditions)
__

KClO

2.) How many grams of
CaCO_{3} are required to produce 6.00 L of CO_{2}?

_{3} à __ CaO +
__ CO_{2}

3.) Determine the
volume of hydrogen gas produced when 0.250 moles of zinc react with

excess HCl._{2} + __ H_{2}

4.) How many liters of nitrogen are required to
combine with 3.0 L of hydrogen in the

following reaction:_{2} + __ H_{2} à __ NH_{3}

5.) How many liters of
oxygen are needed to combine with 7.0 liters of propane in the

following reaction:_{3}H_{8}
+ __ O_{2 }à __
CO_{2} + __ H_{2}O

6.) From the following
reaction:_{4} + __ O_{2}
à __ CO_{2} + __ H_{2}O

_{2} are
formed from 32.0 grams of CH_{4}?

7.) How many grams of
Na are needed to produce 5.0 L of hydrogen?

_{2}O à __ NaOH
+ __ H_{2}

8.) Determine the volume of CO_{2}
produced from burning 0.750 moles of
C.

__ C + __ O_{2} à __ CO_{2}

Answers:
1.) 0.551 L 2.) 26.8
g 3.) 5.60
L 4.) 1.0
L 5.) 35 L

6.) 44.8 L
7.) 10. g
8.) 16.8 L

__DALTON__** ’S LAW
& GRAHAM’S LAW**1. Determine the partial pressure of
each gas in a container with 2.0 moles of N

of O

separate answers for this question.)

2. A mixture of nitrogen
and oxygen has a total pressure of 730 mm Hg. If the nitrogen has a

partial pressure of 420 mm Hg, find the pressure of the
oxygen.

3. At an altitude of
30,000 ft., the total air pressure is only

21.0 % oxygen, what is the partial pressure of oxygen at
this altitude?

4. A mixture of 3 gases have the following pressures: oxygen = 355 mm Hg,
helium = 468

mm Hg, and nitrogen = 560 mm Hg. Find the % of each
gas in the mixture.

5. Compare the rate of
effusion of CH_{4} and CO_{2}. (Give answers to # 5, 6,
& 7 to 3 SF's.)

(Your answers for # 5, 6, &, 7 should read " ___ effuses ___ times faster than ___.")

6. Compare the rate of
effusion of helium and nitrogen.

7. How much faster does
ammonia (NH_{3}) effuse than HCl?

8. An unknown gas effuses
4.0 times faster than O_{2}. Find the molar mass of the
unknown

gas. * What gas could this be?

Answers:
1.) N_{2} = 142 mm Hg, O_{2} = 213 mm Hg, H_{2} = 496
mm Hg 2.) 310 mm Hg

3.) 94.5 mm Hg
4.) O_{2} = 25.7%, He = 33.8 %, N_{2} = 40.5
%

5.) CH_{4} effuses 1.66 times faster than CO_{2}.
6.) He effuses 2.65 times faster than N_{2}.

7.) NH_{3} effuses 1.46 times faster than HCl
8.) 2.0 g/mole

__UNIT 10 REVIEW
WORKSHEET__

1.) Convert the
following pressure measurements to atmospheres.

2.) What are the conditions for gas measurement at STP?

3.) The volume of a sample of
methane gas measures 350. mL
at 27.0 ^{o}C and 810. mm
Hg. What is

the volume (in liters) at -3.0 ^{o}C and 650. mm Hg pressure?

4.) How many grams of nitrogen gas
are contained in a 32.6 liter container at 34.4 ^{o}C
and 579 torr?

5.) A
mixture of four gases in a container exerts a total pressure of 955 mm
Hg. In this container,

there are 4.50 moles of nitrogen
gas, 4.25 moles of carbon dioxide gas, 2.75 moles of hydrogen

gas, and 2.00 moles of oxygen
gas. What is the partial pressure of each gas?

6.) Compare the rates of effusion
of carbon dioxide gas and carbon monoxide gas.

7.) An unknown gas effuses 1.37
times faster than chlorine gas. What is
the molar mass of the unknown gas?

8.) Given the following unbalanced
reaction:

___ C_{5}H_{12} +
___ O_{2} à ___ CO_{2} + ___
H_{2}O

How many liters of oxygen are needed to
produce 45.7 liters of CO_{2}?

9.) Given the unbalanced equation:

___ Mg +
___ O_{2} à ___ MgO

How many liters of oxygen gas are
required to produce 45.8 grams of magnesium

oxide?

10.) An aerosol can contains gases under a pressure of 4.50 atm
at 20.0 ^{o}C. If the can is left on a hot,

sandy beach, the pressure of the
gases increases to 4.80 atm. What is the temperature on the

beach (in ^{o}C)?

1.) (A)
1.5003 atm
(B) 0.600 atm
(C) 1.20 atm

2.) 0 ^{o}C (or 273 K)
& 1 atm 3.) 0.393 L 4.)
27.6 g

5.) N_{2} = 318 mm Hg, CO_{2} = 301 mm Hg, H_{2}
= 195 mm Hg, O_{2} = 141 mm Hg

6.) CO effuses 1.25 times faster than CO_{2}.

7.) 37.8 g/mole 8.)
73.1 L 9.) 12.8 L 10.) 40.0 ^{o}C

Back to
the Unit 10 Worksheets Page