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## PowerPoint Slideshow about 'Mole-Mass and Mole-Volume Relationships' - galvin

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The Mole-Mass Relationship

- To convert the mass of a substance to the number of moles of the substance you have to use the molar mass of an element or compound.
- Mass = # of moles x (mass/1mole)

The Mole-Mass Relationship

- EX: the molar mass of NaCl is 58.5 g/mol, so the mass of 3.00 mol NaCl is calculated:
- Mass of NaCl = 3 mol x (58.5 g/1 mol)
- = 176 g
- When you measure 176 g of NaCl on a balance, you are measuring 3.00 moles of NaCl.

The Mole-Mass Relationship Practice

- What is the mass of 9.45 mol of aluminum oxide (Al2O3)?
- First add up all the masses
- Al = 27g x 2 = 54g
- O = 16g x 3 = 48g
- Al2O3 = 102 g
- Then convert from moles to grams:
- 9.45 mol Al2O3 x (102g/1 mol Al2O3) = 963.9g

The Mole-Mass Relationship Practice

- 16. Find the mass, in grams, of 4.52 x 10-3 mol C20H42.

The Mole-Mass Relationship Practice

- 17. calculate the mass, in grams, of 2.50 mol of iron(II) hydroxide Fe(OH)2.

The Mole-Mass Relationship Practice

- You can calculate the number of moles using the same relationship you use to find the mass of moles by inverting the conversion factor.
- Moles = mass x (1mole/mass)

The Mole-Mass Relationship Practice

- How many moles of iron(III) oxide are contained in 92.2 g of pure Fe2O3?
- Fe2O3 = 159.6 g = 1 mol
- 92.2 g Fe2O3 x (1 mol/159.6 g Fe2O3) = 0.578 mol Fe2O3

The Mole-Mass Relationship Practice

- 18. Find the number of moles in 3.70 x 10-1 g boron.

The Mole-Mass Relationship Practice

- 19. Calculate the number of moles in 75.0 g of dinitrogen trioxide (N2O3)

The Mole-Volume Relationship

- Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.
- Because of variations due to temperature and pressure, the volume of a gas is usually measured at a standard temperature and pressure.

The Mole-Volume Relationship

- Standard temperature and pressure (STP) means a temperature of 0C and a pressure of 101.3 kPa, or 1 atmosphere (atm).

The Mole-Volume Relationship

- At STP, 1 mol or 6.02 x 1023 representative particles, of any gas occupies a volume of 22.4 L.
- The quantity, 22.4 L, is called the molar volume of a gas.

The Mole-Volume Relationship

- The molar volume is used to convert a known number of moles of gas to the volume of the gas at STP.
- Volume of gas = moles of gas x (22.4L/1mol)

The Mole-Volume Relationship

- Determine the volume, in liters, of 0.60 mol SO2 gas at STP.
- 1 mol SO2 = 22.4 L SO2
- Volume = 0.60 mol SO2 x (22.4L/1mol)
- = 13 L SO2

The Mole-Volume Relationship - Practice

- 20. What is the volume of these gases at STP?
- A. 3.20 x 10-3 mol CO2
- B. 3.70 mol N2

The Mole-Volume Relationship - Practice

- 21. at STP, what volume do these gases occupy?
- A. 1.25 mol He
- B. 0.335 mol C2H6

Calculating Molar Mass from Density

- Different gases have different densities. Density of a gas is measured in grams per liter (g/L) and at a specific temperature.
- Molar mass = (grams/L) x (22.4 L/1 mole)

Calculating Molar Mass from Density

- The density of a gaseous compound containing carbon and oxygen is found to be 1.964 g/L at STP. What is the molar mass of the compound?
- Molar mass = (1.964 g/L) x (22.4 L/1 mol)
- = 44 g/mol

Calculating Molar Mass from Density - Practice

- 22. a gaseous compound has a density of 3.58 g/L at STP. What is the molar mass of this gas?

Calculating Molar Mass from Density

- 23. What is the density of krypton gas at STP?

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