part 2: GASES

1. Weak intermolecular forces of attraction

2. They have kinetic energy that produces rapid motion

3. Fill all available spaces

4. Are mostly invisible

5. Compressible

Properties of Gas

1. A gas consists of small particles that are in constant and random motion

2. Gas particles are very small compared with the average distance that separates them

3. Gas particles are constantly colliding with each other and the walls of their container

4. No forces of attraction or repulsion exist between any two gas molecules

5. Average kinetic energy is proportional to the temperature

Kinetic Molecular Theory of Gas

Robert Boyle

Proponent of Boyle’s Law

Mariotte’s Law

Boyle’s Law is also known as?

Boyle’s Law

• Pressure is INVERSELY PROPORTIONAL to Volume

• Constant T and n (amount of Gas)

• Formula: P1V1 = P2V2

• Related to 3rd postulate

P1V1 = P2V2

Formula of Boyle’s Law

Jacque Charles

Proponent of Charles’ Law

Charles’ Law

• Volume is DIRECTLY PROPORTIONAL to Temperature

• Constant P and n (amount of Gas)

• Formula: V1T2 = V2T1

V1T2 = V2T1

Formula of Charles’ Law

Amonton’s Law

Gay Lussac’s Law is also known as?

Joseph Louis Gay Lussac

Proponent of Gay Lussac’s Law

Gay Lussac’s Law

• Pressure is DIRECTLY PROPORTIONAL to Temperature

• Constant V and n (amount of Gas)

• Formula: P1T2 = P2T1

• Related to 5th postulate

P1T2 = P2T1

Formula of Gay Lussac’s Law

Combined Gas Law

• Volume is DIRECTLY PROPORTIONAL to Temperature, and INVERSELY PROPORTIONAL to Pressure

• Constant n (amount of Gas)

• Formula: P1V1/T1 = P2V2/T2

P1V1/T1 = P2V2/T2

Formula of Combined Gas Law

Amedeo Avogadro

Proponent of Avogadro’s Law

Avogadro’s Law

• Volume is DIRECTLY PROPORTIONAL to Amount of Gas

• Constant T and P

• Formula: N1V2 = N2V1

N1V2 = N2V1

Formula of Avogadro’s Law

Ideal Gas Law

Formula: PV = nRT

Application of Ideal Gas Law Equation

• Pressure

• Volume

• Temperature

• Amount of gas

• Weight of gas

• Molecular weight

• Density

PV = nRT

Formula of Ideal Gas Law

• STP = Temp = 0°C / 273K

• Pressure = 1atm

• 1 mole of Gas = 22.4L

Molar Gas Volume

• 0.082057 L.atm/K.mol

• 1.987 cal/mol.K

• 8.3k joules/mol.k

Molar Gas Constant

Real Gas Law

Van der Waals Equation for Real Gases is also known as?

Van der Waals Equation for Real Gases

Modification of Ideal Gas Law

Formula of Van der Waals Equation for Real Gases

John Dalton

Proponent of Dalton’s Law of Partial Pressure

Dalton’s Law of Partial Pressure

• The total pressure of a mixture of gases is equal to the sum of the partial pressure of the individual component gases

• Formula: PTOTAL= P1 + P2 + P3 ……

PTOTAL= P1 + P2 + P3 ……

Formula of Dalton’s Law of Partial Pressure

Thomas Graham

Proponent of Graham’s Law of Effusion

Graham’s Law of Effusion

The rate of Effusion of Gas is INVERSELY PROPORTIONAL to the square root of mass of its particles

William Henry

Proponent of Henry’s Law of Gas Solubility

Henry’s Law of Gas Solubility

At constant Temperature, the amount of dissolved gas is DIRECTLY PROPORTIONAL to the partial pressure of that gas in equilibrium with that liquid

58.33 psi

Sample problem: BOYLE’S LAW

A tire with a volume of 12.41 L reads 47 psi on the tire gauge. What is the new tire pressure if you compress the tire and its new volume is 10 L.

a. 22.32 psi

b. 12.21 psi

c. 32.12 psi

d. 58.33 psi

13.33 mL

Sample problem: BOYLE’S LAW

A syringe has a volume of 20mL. The pressure is 3.0 atm. What must be the final volume to change the pressure to 4.5 atm?

a. 21mL

b. 35.2 mL

c. 22.4 mL

d. 13.33 mL

24.17 L

Sample problem: CHARLES’ LAW

A hot air balloon is under a constant internal pressure. If its volume is 25 liters at a temperature of 30°C, what will be its volume at a temperature at 20°C

a. 24.17 L

b. 16.12 L

c. 35.62 L

d. 42.19 L

12.89 L

Sample problem: COMBINED GAS LAW

A 10 L air sample has a pressure of 800 torr at -50°C. What will be the volume of air be at STP?

2.17 mol

Sample problem: AVOGADRO’S LAW

4L of container is known to contain 0.965 mol of gas. More gas is then added to the container until it reaches a final volume of 9.00 L. Assuming the pressure and temperature of the gas remain constant. Calculate the number of moles of gas added to the container.

12.34 atm

Sample problem: DALTON’S LAW

What is the total pressure of a 10 L gas tank containing 4 moles of Helium and 1.1 mole of Oxygen gas @ 295K?

32g

Sample problem:

Determine the weight of the unknown gas at STP and its molecular weight is 32 g/mole

50.27g/mol

Sample problem:

Find the molecular weight of the unknown gas if its density is 5.71g/L having a pressure of 2.88 atm in 309 K

1. Anesthetic Gases

2. Compressed and Liquefied Gases

3. Gas Sterilant

Pharmaceutical Gases

1. Nitrous oxide

2. Halothane

3. Isoflurane

Anesthetic Gases

Nitrous oxide

Most widely used anesthetic gas

Halothane

Anesthetic of choice for children and asthmatic patients

Isoflurane

Anesthetic of choice for neurosurgery

1. Nitrogen

2. Carbon dioxide

Compressed Gas

1. Butane

2. Isobutane

3. Propane

Liquefied Gas

Gas sterilant

Used for sterilization of heat-labile substances

1. Ethylene oxide

2. Formaldehyde gas

Gas sterilant