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Transcript of chemistry -1/Chapter 10/chem 10-2...solve chemistry problems. 10.2 • The Mole–Mass Relationship...
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Chemistry 10-2
Mole–Mass and Mole–Volume Relationships
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• 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.
10.2
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• The Mole–Mass Relationship – How do you convert the mass of a substance to
the number of moles of the substance?
10.2
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• Use the molar mass of an element or compound to convert between the mass of a substance and the moles of a substance.
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• The Mole–Volume Relationship – What is the volume of a gas at STP?
10.2
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• Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.
10.2
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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 – a pressure of 101.3 kPa, or 1 atmosphere (atm).
10.2
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• At STP, 1 mol or, 6.02 × 1023 representative particles, of any gas occupies a volume of 22.4L. – The quantity 22.4 L is called the molar volume of a
gas.
10.2
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– Calculating Volume at STP
10.2
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– Calculating Molar Mass from Density
10.2
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The Mole Road Map 10.2
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10.2
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The Mole Road Map 10.2
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The Mole Road Map 10.2
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