Essay on Ideal Gas Law and Gas

Submitted By Victoria-Garza
Words: 1871
Pages: 8
Open Document
Gas Laws

Elements that exist as gases at 250C and 1 atmosphere

Physical Characteristics of Gases
•

Gases assume the volume and shape of their containers.

•

Gases are the most compressible state of matter.

•

Gases will mix evenly and completely when confined to the same container.

•

Gases have much lower densities than liquids and solids.

Force
Pressure = Area

Units of Pressure
1 pascal (Pa) = 1 N/m2
1 atm = 760 mmHg = 760 torr
1 atm = 101,325 Pa
Barometer

10 miles

4 miles
Sea level

0.2 atm

0.5 atm
1 atm

As P (h) increases

V decreases

Boyle’s Law

P  1/V
P x V = constant
P1 x V1 = P2 x V2

Constant temperature
Constant amount of gas

A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

P1 x V1 = P2 x V2
P1 = 726 mmHg

P2 = ?

V1 = 946 mL

V2 = 154 mL

P1 x V1
726 mmHg x 946 mL
P2 =
=
= 4460 mmHg
154 mL
V2

As T increases

V increases

Variation of gas volume with temperature at constant pressure.

Charles’ &
Gay-Lussac’s
Law

VT
V = constant x T
V1/T1 = V2/T2

Temperature must be in Kelvin
T (K) = t (0C) + 273.15

A sample of carbon monoxide gas occupies 3.20 L at
125 0C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant?

V1/T1 = V2/T2
V1 = 3.20 L

V2 = 1.54 L

T1 = 398.15 K

T2 = ?

V2 x T1
T2 =
=
V1

1.54 L x 398.15 K
3.20 L

= 192 K

Avogadro’s Law
V  number of moles (n)
V = constant x n
V1/n1 = V2/n2

Constant temperature
Constant pressure

Ammonia burns in oxygen to form nitric oxide (NO) and water vapor. How many volumes of NO are obtained from one volume of ammonia at the same temperature and pressure?

4NH3 + 5O2
1 mole NH3

4NO + 6H2O
1 mole NO

At constant T and P
1 volume NH3

1 volume NO

Ideal Gas Equation
1
Boyle’s law: V (at constant n and T)
P
Charles’ law: V  T(at constant n and P)
Avogadro’s law: V n(at constant P and T) nT V
P

nT nT V = constant x
=R
P
P

R is the gas constant

PV = nRT

The conditions 0 0C and 1 atm are called standard temperature and pressure (STP).
Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L.

PV = nRT
(1 atm)(22.414L)
PV
R=
=
nT
(1 mol)(273.15 K)
R = 0.082057 L • atm / (mol • K)

What is the volume (in liters) occupied by 49.8 g of HCl at STP?
T = 0 0C = 273.15 K

PV = nRT nRT V=
P

P = 1 atm
1 mol HCl n = 49.8 g x
= 1.37 mol
36.45 g HCl

1.37 mol x 0.0821
V=
V = 30.6 L

L•atm mol•K 1 atm

x 273.15 K

Argon is an inert gas used in lightbulbs to retard the vaporization of the filament. A certain lightbulb containing argon at 1.20 atm and 18 0C is heated to
85 0C at constant volume. What is the final pressure of argon in the lightbulb (in atm)?

PV = nRT

n, V and R are constant

nR
= P = constant
T
V
P1
P2
=
T1
T2

P1 = 1.20 atm
T1 = 291 K

P2 = ?
T2 = 358 K

T2
= 1.20 atm x 358 K = 1.48 atm
P2 = P1 x
291 K
T1

Density (d) Calculations
PM
m d= =
V
RT

m is the mass of the gas in g
M is the molar mass of the gas

Molar Mass (M ) of a Gaseous Substance dRT M=
P

d is the density of the gas in g/L

Gas Stoichiometry

What is the volume of CO2 produced at 370 C and 1.00 atm when 5.60 g of glucose are used up in the reaction:
C6H12O6 (s) + 6O2 (g)

6CO2 (g) + 6H2O (l)

g C6H12O6

mol C6H12O6

5.60 g C6H12O6 x

6 mol CO2
1 mol C6H12O6 x = 0.187 mol CO2
180 g C6H12O6
1 mol C6H12O6

V=

nRT
=
P

mol CO2

V CO2

L•atm x 310.15 K mol•K 1.00 atm

0.187 mol x 0.0821

= 4.76 L

Dalton’s Law of Partial Pressures

V and T are constant

P1

P2

Ptotal = P1 + P2

Consider a case in which two gases, A and B, are in a container of volume V.

nART
PA =
V

nA is the number of moles of A

nBRT
PB =
V

nB is the number of moles of B

PT = PA + PB
PA = XA PT

nA
XA = nA + nB
PB = XB PT
Pi = Xi PT

nB
XB = nA + nB

A sample of natural gas contains 8.24 moles of CH4,
0.421 moles of C2H6, and 0.116 moles of C3H8. If the total pressure of the gases is 1.37
Show More

Related Documents: Essay on Ideal Gas Law and Gas

Essay on Ideal Gas Law lab

still a few scattered bubbles and all of the Alka-Seltzer has gone into the water. The balloon is standing erect and slightly firm to the touch. There is water inside the balloon. The bubbling has stopped. When the balloon was cut a small whoosh of gas could be heard escaping. The balloon returned to normal size. On the inside of the balloon there are trace remains of Alka-Seltzer powder. Mass measurements: Mass (±.05g) Mass of flask with water, balloon, Alka-Seltzer 396.8g (±.05g) Mass of items…

Words 579 - Pages 3

Things: Ideal Gas Law and Temperature Essay

Exploring the Properties of Gas Shawna Hendricks CHM 144 C Robert Baum Colleen Heffner and Andrew Flannery Abstract: The hypothesis of whether or not the relationships between the properties of gases will all be direct is experimented. This was done by experimenting three variables of properties of gases such as temperature, pressure, and volume. Temperature and pressure were tested together while volume was kept constant, then the relationship…

Words 2055 - Pages 9

Gas Law Essay

Gas Laws -study the relationships that exist between pressure, volume, temperature and amount (moles) of gas. 1. Boyle’s Law * Pressure-volume relationship * At constant temperature and amount, the pressure and volume of a gas are inversely proportional. * As pressure increases, volume decreases. * P1V1=P2V2 2. Charles’ Law * Temperature-volume relationship * At constant pressure and amount, the temperature and volume of a gas are directly proportional.…

Words 518 - Pages 3

Expt 0 Essay example

experiment the ideal gas law and the van der Waals equation were examined. In Part 1, the gas constant was determined by graphing P vs 1/V for data collected using nitrogen gas. The equation of the line was y= 2.7817x- 0.2592. The gas constant was 0.93 ± 0.014 L*atm/mol*K. In Part II, six different isotherms were graphed assuming ideal gas behavior. In Part III, six different isotherms were graphed using the van der Waals equation. Using the same volume, the pressure under ideal gas behavior was higher…

Words 1178 - Pages 5

Lab 1 The Determination of R Essay

The Determination of R: The Gas-Law Constant Izabella D’Onofrio Conducted on: January 24, 2015 Abstract An experiment was performed to determine “R”, the gas-law constant, using both the ideal gas law equation and the van der Waals equation. An ideal gas is considered a hypothetical gas whose pressure, volume, and temperature behavior correlates to the ideal gas equation, PV=nRT (Brown, et al. 2012). Using an apparatus involving a test tube and large beaker with rubber stoppers and…

Words 1157 - Pages 5

Physics 158 matter notes Essay

GASES  IDEAL GAS: attractive forces between molecules are assumed negligible, but they can interact through collisions.  Pressure of gas on container is due to collisions of gas molecules against container walls. IDEAL GAS LAW where n = number of moles of gas molecules R = Universal Gas Constant = 8.32 J/(mol.K) T = Absolute Temperature (K) P = Absolute (or Total) Pressure Note: T(K) = T (C) + 273.15 SPECIAL CASES Often some variable is…

Words 327 - Pages 2

Essay on Lab report 2 Edition

scientific laws in lab, it is important to understand the relationship between the different variables at play. Using the Ideal Gas Law the following behaviors, Pressure (P), Volume (V), Temperature (T), and quantity in moles (n) relationships are examined between each other. However, before using these terms, the assumptions under the ideal gas law—that molecules don’t interact when in a gas state and that volume occupied by molecules is negligible—were taken into consideration The ideal gas laws states…

Words 1882 - Pages 8

Fractures of the Thoracic Spine Essay

   A gas consists of very small particles called molecules that are in constant random motion The molecules collide with each other and with the walls of the containing vessel The collisions are considered to be elastic so that there is no kinetic loss due to collision The average molecular kinetic energy is proportional to temperature (in Kelvin) of the gas The size of the molecules is negligibly small compared with the space they occupy 4 Emprical Laws of Gases Boyle’s Law  Charles’…

Words 1452 - Pages 6

Essay about Determining Molar Volume of a Gas

Volume of Gas Using Magnesium and Hydrochloric Acid and Demonstrating Boyles Law Taylor Payne Abstract: In this experiment we combined a strip of magnesium with hydrochloric acid in a buret and measured the amount of hydrogen gas the reaction produced. We also tracked the pressure inside a syringe as the volume of the syringe increased and decreased. Introduction: The moles and density of the hydrogen gas that is produced in this experiment can be calculated using the combined gas law equation…

Words 595 - Pages 3

Essay Gfghvh

Avogadro’s Law Multiple Choice Questions 1. How many atm of gas did you add to the flask? A. 1 atm B. 3 atm C. 4 atm D. 2 atm 2. What was the volume of the flask? E. 100 mL F. 120 mL G. 150 mL H. 88 mL 3. How many grams of propane were there in 1 atm? Choose the closest answer. I. 0.735 g J. 0.274 g K. 0.664 g L. 0.232 g 4. How many grams of butane were there in 1 atm of gas? Choose…

Words 1024 - Pages 5