MOLAR VOLUME. molar volume What is the volume of a gas at STP, if it contains 10.4 moles? What is the volume of carbon dioxide gas (STP) if the.

MOLAR VOLUME

MOLAR VOLUME

MOLAR VOLUME

MOLAR VOLUME

molar volume • What is the volume of a gas at STP, if it

contains 10.4 moles?

• What is the volume of carbon dioxide gas (STP) if the mass is 400 grams?

• What is the mass of 500 liters of oxygen at STP?

H2 + O2 H2O• How many liters of oxygen are required when

making 180 grams of water.• BCA table is required. O2 to H2O

•ONE MORE EQUATION

Ideal Gas Equation

Charles’ law: V T(at constant n and P)

Avogadro’s law: V n(at constant P and T)

Boyle’s law: V (at constant n and T)1P

V nT

P

V = constant x = RnT

P

nT

PR is the gas constant

PV = nRT

The conditions 0 0C and 1 atm are called standard temperature and pressure (STP).

PV = nRT

R = PVnT

=(1 atm)(22.414L)

(1 mol)(273.15 K)

R = 0.0821 L • atm / (mol • K)

Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L.

pressure must be in atmospheres (atm)

The conditions 0 0C and 1 atm are called standard temperature and pressure (STP).

PV = nRT

R = PVnT

=(760 mmHg)(22.4L)

(1 mol)(273 K)

Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L.

pressure must be in: mm Hg

“R” value

when using mm Hg

when using atmatm

What is the volume (in liters) occupied by 49.8 g of HCl at STP?

PV = nRT

V = nRTP

T = 0 0C = 273 K

P = 1 atm

n = 49.8 g x 1 mol HCl36.5 g HCl

= 1.37 mol

V =1 atm

1.37 mol x 0.0821 x 273 KL•atmmol•K

V = 30.6 L

EXPANDING ON PV = nRT

• Determining the GRAMS of a gas (not at STP) when given the VOLUME

• Determining the VOLUME of a gas (not at STP) when given the GRAMS

REMEMBER we must think that grams (or particles “atoms” or molecules) are the same

as MOLES

What is the number of grams of oxygen in the following?

• P = 1.5 atm

• V = 24.0 L

• T = 10oC

• n = ?

• R = 0.0821 L atm

mol K

• n (# of moles) is the unknown.

• Then convert to grams

How many liters of carbon dioxide are in the following condition?

• P = 740 mm Hg• T = 30oC• 440 grams

• Convert grams to moles

• then use the IDEAL GAS LAW

• R = 0.0821 L atm

mol K

Aluminum combines with oxygen to form Aluminum oxide. How many liters of oxygen are

formed with 270 grams of aluminum at a pressure of 1 atm and a temperature of 10oC?

MOLAR VOLUME

MOLAR VOLUME

MOLAR VOLUME

MOLAR VOLUME

molar volume • What is the volume of a gas at STP, if it

contains 10.4 moles?

• What is the volume of carbon dioxide gas (STP) if the mass is 400 grams?

• What is the mass of 500 liters of oxygen at STP?

H2 + O2 H2O• How many liters of oxygen are required when

making 180 grams of water.• BCA table is required. O2 to H2O

•ONE MORE EQUATION

Ideal Gas Equation

Charles’ law: V T(at constant n and P)

Avogadro’s law: V n(at constant P and T)

Boyle’s law: V (at constant n and T)1P

V nT

P

V = constant x = RnT

P

nT

PR is the gas constant

The conditions 0 0C and 1 atm are called standard temperature and pressure (STP).

PV = nRT

R = PVnT

=(1 atm)(22.414L)

(1 mol)(273.15 K)

R = 0.0821 L • atm / (mol • K)

Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L.

pressure must be in atmospheres (atm)

What is the volume (in liters) occupied by 49.8 g of HCl at STP?

PV = nRT

V = nRTP

T = 0 0C = 273 K

P = 1 atm

n = 49.8 g x 1 mol HCl36.5 g HCl

= 1.37 mol

V =____ atm

_____ mol x 0.0821 x ____ KL•atmmol•K

V =________

What is the number of grams of oxygen in the following?

• P = 1.5 atm

• V = 24.0 L

• T = 10oC

• n = ?

• R = 0.0821 L atm

mol K• n (# of moles) is the

unknown.• Then convert to grams

How many liters of carbon dioxide are in the following condition?

• P = 740 mm Hg• T = 30oC• 440 grams

• Convert grams to moles

• then use the IDEAL GAS LAW

• R = 0.0821 L atm

mol K