1. A gas sample occupies a volume of 2.5 L at a pressure of 1.5 atm. What would be the volume of the gas if its pressure is reduced to 1 atm at the same temperature?
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![GAS LAW PROBLEM SET
Directions: Read the information given in each gas law and answer the following problems with complete solution in
GRESA format.
A. BOYLE'S LAW
In 1662, Robert Boyle reported that the volume of gas decreased with increasing
pressure. Within the limits of his experimental accuracy, he postulated the relationship existing
between pressure and the volume was an inverse proportionality at constant temperature.
Boyle's Law Equation: P1V1 = P2V2
Sample Problem:
Calculate the final volume of a gas if the pressure of a 4.0 L sample is changed from 2.5 atm to 5.0 atm.
Given: V= 4.0L; P 2.5 atm; P, = 5.0 atm
Required: V,
Equation: V2 =
P2
Solution:
(25 alm)(4.OL)
V2 =
= 2L
5.0alm
Answer:
V2=2L
1. A gas sample occupies a volume of 2.5 L at a pressure of 1.5 atm. What would be the volume of the gas if its
pressure is reduced to 1 atm at the same temperature?
2. The gas inside a balloon has a volume of 15.0L at a pressure of 2.0 atm. Calculate the pressure of the gas if its
volume is compressed to 10.0L at the same temperature.
B. CHARLES' LAW
Gas when heated at constant pressure will expand, and contract when cooled. This
relationship was studied by Jacques Charles. He stated that at constant pressure, the
volume of a given quantity of gas varies directly with the absolute temperature (K).
V1
Charles' Law Equation:
T1
V2
=
Note: The temperature must be expressed in Kelvin (K).
-
T2
Sample Problem:
At 30°C, the volume of a sample of air was 5.8 L. What would be the volume of the air sample if it is heated to
60°C at the same pressure?
Given: T, = 30°C + 273 = 303 K; V, = 5.8L; T, = 60°C + 273 = 333 K
Required: V,
Equation: V1T2 = V2T1 ; V2 =
Solution:
(58L(333
303X
= 6.37 L
Vz =
Answer:
Va- 6.37 L
3. A given amount of oxygen gas has a volume of 25.0 L at a temperature of 370C and a pressure of 1.0 atm. At
what temperature would this gas occupy a volume of 22.0 L at a pressure of 1.0 atm?
4. A gas syringe contains 56.05 milliliters of a gas at 315.1 K. Determine the volume in L that the gas will occupy if
the temperature is increased to 380.5 K.
c. GAY-LUSSAC'S LAW
Gay Lussac's law defines the relationship between the pressure and temperature
of a gas. According to the law, when volume is held constant, the pressure of an ideal gas
is directly proportional to its temperature.
P2
;Note: The temperature must be expressed in Kelvin (K).
T2
Gay-Lussac's Equation:
Sample Problem:
A 30.0 L sample of nitrogen inside a rigid, metal container at 20.0 *C is placed inside an oven whose temperature
is 50.0 "C. The pressure inside the container at 20.0 °C was at 3.00 atm. What is the pressure of the nitrogen after its
temperature is increased to 50.0 "C?
Given: T, = 20.0'C + 273 = 293 K; P, = 3.00 atm; T= 50.0°C + 273 = 323 K
Required: P2
Equation: PT2 = PT : Pz=
Solution:
P2 =
(3.00 atm)(323)
293
= 3.31 atm
Answer:
Pa= 3.31 atm
5. Calculate the final pressure inside a scuba tank after it cools from 1.00x10 "C to 25.0 "C. The initial pressure in the
tank is 130.0 atm.
6. If a gas in a closed container is pressurized from 15.0 atm to 16.0 atm and its original temperature was 298 K,
what would the final temperature of the gas be in degrees Celsius? Note: convert from K to "C and then round off.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe3b91870-9327-4bc9-a137-0ace00bec9d0%2F00ef75ce-9893-493a-9a66-6123abac0774%2Fztpx6bt_processed.jpeg&w=3840&q=75)
![D. COMBINED GAS LAW
The combined gas law combines the first three gas law: Boyle's Law, Charles'
Law, and Gay-Lussac's Law. It states that the ratio of the product of pressure and
volume and the absolute temperature of a gas is equal to a constant.
Combined Gas Law Equation: 11 = 22; Note: The temperature must be expressed in Kelvin (K).
Sample Problem:
Find the volume of a gas at STP when 2.00 L is collected at 745.0 mmHg and 25.0 °C.
Given: P, = 745.0 mmHg = 745.0 torr = 0.98 atm; V, = 2.00 L; T, = 25 + 273 = 298 K; STP (P2 = 760.0 mmHg = 760.0
torr = 1 atm; T2 = 273 K)
Required: V2
P,V,T2
Equation: PV,T2 = P2V2T1 ; V2 =
Solution:
(0.98 atm)(2.00L)(273 K)
V2 =
= 1.80 L
(1 atm)(298 K)
Answer:
V2 =1.80 L
7. A gas takes up a volume of 17 L, has a pressure of 2.3 atm, and a temperature of 299 K. If the temperature
raised to 350 K and pressure is lowered at 1.5 atm, what is the new volume of gas?
8.
If you have 2.9 L of gas at a pressure of 5 atm and a temperature of 50°C, what will be the temperature in Kelvin
of the gas if you decrease the volume to 2.4 L and pressure to 3 atm?
E. IDEAL GAS LAW
The Ideal Gas Law was created to show the relationship between
pressure, volume, number of moles of gas and temperature. It shows the
equation of a hypothetical ideal gas.
Ideal Gas Law Equation: PV = nRT; Note: The temperature must be expressed in Kelvin (K).
Sample Problem:
How many moles of gas are contained in 890.0 ml at 21°C and 750 mmHg?
atm •L
mol •K
Given: P = 750 mmHg = 750 torr = 0.99 atm; V = 890 ml = 0.89 L; R = 0.0821 T = 21°C + 273 = 294 K
Required: n
PV
Equation: n =
RT
Solution:
(0.99 atm) (0.89 L)
n =
= 0.037 mol
(0.0821 (294 K)
mol-K
Answer:
n=0.037 mol
9. Calculate the volume if 3.00 moles of a gas will occupy at 24°C and 762.4 mmHg.
10. What is gas' temperature in Kelvin when it has a volume of 25 L, 203 mol, and a pressure of 143.5 atm?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe3b91870-9327-4bc9-a137-0ace00bec9d0%2F00ef75ce-9893-493a-9a66-6123abac0774%2Fp8glxf9_processed.jpeg&w=3840&q=75)
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