Intro to GasesBoyle’s Law Lab

Chemistry 4/16/15

Drill

New packet!

How are gases different from solids and liquids?

How can you describe a gas?

HW: Finish 13-2 Practice Probs (pg. 2)

Objectives

IWBAT Describe gases by their properties Discover the mathematical relationships in

Boyle’s Law.

Agenda

Drill

Intro to Gases Notes (front of note sheet)

Pressure conversions

Closure

Physical Characteristics

of GasesKinetic Molecular Theory

Kinetic Molecular Theory of Gases

The kinetic molecular theory of matter (KMT) is based on the idea that particles of gases are always in motion.

The KMT assumes that a gas is ideal: An ideal gas is an imaginary gas that fits all the

assumptions of KMT. Ideal gases are NOT real, but gases behave like ideal

gases when pressure is not high and temperature is not low. What happens when pressure is high or when

temperature is low?

Assumptions of KMT

Gases consist of large numbers of tiny particles that are far apart from each other relative to their size.

Collisions between gas particles and other things are completely elastic -- no energy is lost.

Gas molecules are in constant, rapid motion.

There is no attraction or repulsion between gas molecules.

The average kinetic energy of gas molecules depends on the temperature of the gas.

Physical Properties of

Gases Expansion -- no definite shape or volume

Fluidity -- flows freely

Low density

Compressibility -- may be crowded together

Diffusion -- spontaneous mixing of two gases

Effusion -- particles under pressure can leak out of a tiny opening

Standard Temperature and Pressure (STP): 1 atm, 273K

Units and Equipment for Measuring Gases

Units: Pressure:

Atmospheres (atm)

Pascals (Pa) Millimeters of

mercury (mmHg) Volume

Liters or milliliters (L or mL)

Amount of the Gas Moles (mol)

Temperature Kelvin (K) NOT Celsius or

Fahrenheit

Equipment: Pressure:

Pressure gauge Barometer

What is air pressure?

Air pressure is the weight of the air pressing down on an object.

Air presses in all directions, with the same amount – about 760 mmHg.

Conversions

We will frequently need to convert between different measurements, especially for pressure: 1 atm = 101.325 kPa = 760 mmHg = 14.69

lb/in2

Temperature: K = °C + 273.15 °C = K - 273.15

Practice with Conversion

Let’s practice with 13-2 Practice Problems #1-8 – conversions of pressure measurements.

Let’s review

The Gas Laws: Boyle’s and

Charles’ Boyle’s Law:

Pressure and Volume of a gas are indirectly proportional to each other.

As pressure goes up, volume goes down (and visa-versa)

P1V1 = P2V2

Charles’ Law: Volume and Temperature of a gas are

directly proportional to each other. As temperature goes up, volume goes up

(and visa-versa) V1/ T1 = V2 / T2

The Gas Laws: Gay-Lussac’s and

Combined

Gay-Lussac’s Law: Pressure and temperature of a gas

are directly proportional to each other.

As temperature goes up, so does the pressure (and visa-versa)

P1 / T1 = P2 / T2

The Combined Gas Law: P1V1 = P2 V2 T1 T2

The Gas Laws:Dalton’s and

Graham’s

Dalton’s Law of Partial Pressures The pressures of mixed gases add together. PTotal = P1 + P2 + P3 + ...

Graham’s Law Compares the rates of diffusion of any two gases using the

following equation: Ms. Bloedorn will write it on the board

Moles and Gases As you increase the amount of a gas (moles), the

volume increases too.

Avogadro’s Law: V1 = V2 n1 n2 It is rarely used in this form.

Ideal Gas Law: PV = nRT R = 0.0821 L • atm mol • K

Moles and Gases, cont.

If all gases act the same way, would the volume of a mole of any gas be the same at STP? YES!

The standard molar volume of a gas (volume of 1 mol at STP) is 22.4 L.

22.4 L/mol!

Closure

State Boyle’s Law in your own words.