chemistry

Mole–Mass and Mole–Volume Relationships 10.2 Mole–Mass and Mole–Volume Relationships How can you guess the number of jelly beans in a jar? You estimate the size of a jelly bean and then estimate the dimensions of the container to obtain its volume. In a similar way, chemists use the relationships between the mole and quantities such as mass, volume, and number of particles to solve chemistry problems.

The Mole–Mass Relationship 10.2 The Mole–Mass Relationship The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance?

The Mole–Mass Relationship 10.2 The Mole–Mass Relationship Use the molar mass of an element or compound to convert between the mass of a substance and the moles of a substance.

10.5 These aluminum satellite dishes at the National Radio Astronomy Observatory near Soccoro, New Mexico are naturally protected from corrosion by the formation of a thin film of aluminum oxide (Al2O3).

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for Sample Problem 10.5 Problem Solving 10.16 Solve Problem 16 with the help of an interactive guided tutorial.

10.6 Rust weakens an iron chain.

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for Sample Problem 10.6 Problem Solving 10.18 Solve Problem 18 with the help of an interactive guided tutorial.

The Mole–Volume Relationship 10.2 The Mole–Volume Relationship The Mole–Volume Relationship What is the volume of a gas at STP?

The Mole–Volume Relationship 10.2 The Mole–Volume Relationship Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. In each container, the volume occupied by the gas molecules is small compared with the container’s volume, so the molecules are not tightly packed. a) The molecules in this container are small. b) This container can accommodate the same number of larger molecules.

The Mole–Volume Relationship 10.2 The Mole–Volume Relationship The volume of a gas varies with temperature and pressure. Because of these variations, the volume of a gas is usually measured at a standard temperature and pressure. Standard temperature and pressure (STP) means a temperature of 0°C and a pressure of 101.3 kPa, or 1 atmosphere (atm).

The Mole–Volume Relationship 10.2 The Mole–Volume Relationship At STP, 1 mol or, 6.02  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. This box, with a volume of 22.4 L, holds one mole of gas at STP.

The Mole–Volume Relationship 10.2 The Mole–Volume Relationship Calculating Volume at STP

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for Sample Problem 10.7 Problem Solving 10.20 Solve Problem 20 with the help of an interactive guided tutorial.

The Mole–Volume Relationship 10.2 The Mole–Volume Relationship Calculating Molar Mass from Density

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for Sample Problem 10.8 Problem Solving 10.22 Solve Problem 22 with the help of an interactive guided tutorial.

10.2 The Mole Road Map The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?

10.2 The Mole Road Map The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?

10.2 The Mole Road Map The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?

The Mole Road Map 10.2 The Mole Road Map The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?

Simulation 10 Simulation 10 Use the mole road map to convert among mass, volume, and number of representative particles.

10.2 Section Quiz. 10.2.

10.2 Section Quiz. 1. Calculate the mass in grams of a sample containing 1.85 x 1034 molecules of water. 3.07 x 1010 g 5.53 x 1011 g 188 g 8.46 x 103 g

10.2 Section Quiz. 2. Calculate the number of moles in a spoonful of table sugar (C12H22O11) having a mass of 10.5 g. 32.6 mol 3.59  103 mol 3.07  10–3 mol 1.85  1022 mol

10.2 Section Quiz. 3. What is the volume of 0.35 mol of oxygen gas at STP? 32 L 64 L 7.8 L 16 L

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