Quiz 8: Properties and Laws of Gases

1. There must be space in between gas molecules

2. Gas molecules move rapidly

3. Gas molecules collide w/ the container

4. Gas moves at a faster and higher temperature

What are the 4 general properties of gases?

Gas particles are in constant, random and rapid motion

Kinetic Molecular Theory of Gases (KMT):

A gas consists of an extremely large number of very tiny particles that are in ___________, ____________and ____________ motion

constant motion

Kinetic Molecular Theory of Gases (KMT):

All matter is made up of tiny particles that are in ______________

Temperature (Temp is related to KE)

Kinetic Molecular Theory of Gases (KMT):

The average kinetic energy of gas particles is directly proportional to the _______________ of the gas

Individual gas particles

Kinetic Molecular Theory of Gases (KMT):

The volume of _______________ are negligible compared to the volume of the whole gas

- random

- straight lines

Kinetic Molecular Theory of Gases (KMT):

The motion of gas particles is ___________, and they move in ______________ until they collide with other particles or the walls of their container

- Faster

- Increases

As temperature increases, gas molecules move at a ______________ pace and kinetic energy _______________

- Heavier

- Slower

If temperature remains constant, gas molecules become ___________ causing them to move ____________ while kinetic energy remains constant

- Atmospheric pressure

- barometer

_____________________ is the pressure exerted by air molecules colliding with objects and is measured using a _______________

1 atm = 101325 Pa = 760 torr = 760 mmHg = 14.6959 PSi

Unit conversions for pressure:

____atm = _________ Pa = __________ torr = _________ mmHg = _________ PSi

1 atm = 101325 Pa = 760 torr = 760 mmHg = 14.6959 PSi

List the unit conversions for pressure

824 mmHg x (1 atm/760 mmHg) = 1.08 atm

Convert 824 mmHg to atm

824mmHg x (101325 Pa/ 760mmHg) x (1KPa/103 Pa) = 110. KPa

Convert 824 mmHg to KPa

1. Boyles law

2. Charles law

3. Avogadros law

4. Amontons law

What are the 4 Gas laws?

Boyles gas law

The relationship below is described by the ______________ gas law:

P (pressure) ∝ 1/V (volume) If T (temperature) and n (moles) are constant

Charles gas law

The relationship below is described by the ______________ gas law:

V ∝ T If P and n are constant

Avogadros gas law

The relationship below is described by the ______________ gas law:

V ∝ n If P and T are constant

Amontons gas law

The relationship below is described by the ______________ gas law:

P ∝ T If vtn are constant

Boyles law

Gas law:

_______________ states that pressure increases as volume of the container decreases

Charles law

Gas law:

_______________ states that volume increases as temperature increases

(volume decreases as temperature decreases)

Avogadros law

Gas law:

_______________ states that volume increases as moles increases

Amontons law

Gas law:

_______________ states that pressure increases as temperature increases

PV/T (Pressure x Volume/temperature)

The Combined Gas Law states that for a fixed amount of gas, constant = _____________

(P1V1)/ T1 = (P2V2)/ T2

What equation is used in the Combined Gaw Law?

T(K) = T(°C) + 273.15

The Combined Gas Law states that temperature needs to be converted to kelvin when solving for

(P1V1)/ T1 = (P2V2)/ T2

What equation is used to convert Celsius to kelvin?

Pressure and Volume

The Combined Gas Law states that __________ and __________ can be in any units as long as they are the same when solving for

(P1V1)/ T1 = (P2V2)/ T2

(P1V1)/ T1 = (P2V2)/ T2

(785 x 0.879)/ 295K = (337 x V2)/ 226K

V2 = 1.576

Find the final volume using the combined gas law:

P1 = 785mmHg

T1 = 22 degrees Celsius

V1 = 0.879L

P2 = 387mmHg

T2 = -47 degrees Celsius

P1V1 = P2V2

22.5 atm (760 torr/ 1 atm) = 17100 torr

(17100 x 41.0) = (5.15 x V2)

V2 = 136000 L

Find the final volume using the combined gas law:

P1 = 22.5 atm

V1 = 41.01L

T1 = T2

P2 = 5.15 torr

T(k) = 25 degree Celsius + 273K = 298K

(1.51 x 455)/298 k = (2.00 x 222)/ T2

2.305 T2 = 193k - 273

T2 = -80 degrees Celsius

Find the final temperature using the combined gas law:

P1 = 1.51 atm

V1 = 455mL

T1 = 25 degrees Celsius

P2 = 2.00 atm

V2 = 222mL

PV = nRT

What equation is used in the Ideal Gas Law?

R is the Ideal gas constant (0.08206 L atm/mol K)

What does the R stand for:

PV = nRT

(atm x L) = (mol x R x K)

The Ideal gas law states that the units for PV = nRT needs to be __________ = ___________

Standard temperature is 273K and standard pressure is 1 atm

What is the standard temperature and pressure (STP) values?

22.4 L

What is the molar volume of 1 mol of gas at STP?

2.00mol x (22.4L/ 1 mol) = 44.8L

What is the molar volume of 2 mol of gas at STP?

PV = nRT

n = 1.22g x (1 mol/ 4.0026g) = 0.305 mol

P (5.50L) = (0.305mol x 0.08206 x 298K)

P = 1.36 atm

We have 1.22g of He gas at 25 degrees Celsius in a 5.50L drum. What is the pressure of He gas?

PV = nRT

(1.00atm x 2.00L) = n (0.08206 x 273K)

n = 0.0893 mol

0.0893 mol x (16.04g/1 mol) = 1.43g

Solve for the grams of CH4 (16.04 g/mol)

V = 2.00L

T = 273 K

P = 1.00 atm

Real gas, Ideal gas is shown as a straight linear line (hence the assumption that the mid-section of this graph behaves as ideaL)

The graph shown is a visual of ____________