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Questions and Answers
What does Avogadro's Law state about gases at a constant temperature and pressure?
What does Avogadro's Law state about gases at a constant temperature and pressure?
- The volume of a gas decreases as the pressure increases.
- The volume of a gas is inversely proportional to its temperature.
- The volume of a gas is directly proportional to the number of moles. (correct)
- The volume of a gas is constant regardless of the number of moles.
What did Gay-Lussac conclude regarding the volumes of gases in chemical reactions?
What did Gay-Lussac conclude regarding the volumes of gases in chemical reactions?
- Gaseous reactants and products have ratios of whole numbers. (correct)
- The volume of gas only depends on temperature.
- Gases react in equal volumes.
- The volumes of gases are always unpredictable.
How did Avogadro's hypothesis contribute to the understanding of gas behavior?
How did Avogadro's hypothesis contribute to the understanding of gas behavior?
- It proposed that gas volume is not affected by pressure.
- It indicated that the temperature of a gas has no effect on its volume.
- It claimed that the density of gases is uniform under all conditions.
- It suggested equal volumes of gases contain the same number of particles. (correct)
What relationship does the formula $ rac{n_1}{n_2} = rac{V_1}{V_2}$ represent in Avogadro's Law?
What relationship does the formula $ rac{n_1}{n_2} = rac{V_1}{V_2}$ represent in Avogadro's Law?
What occurs when more gas enters a container at constant temperature?
What occurs when more gas enters a container at constant temperature?
At STP, how much volume does 1.0 mol of carbon dioxide gas occupy?
At STP, how much volume does 1.0 mol of carbon dioxide gas occupy?
Which of the following laws did Gay-Lussac's observations lead to?
Which of the following laws did Gay-Lussac's observations lead to?
What must remain constant for Avogadro's Law to apply?
What must remain constant for Avogadro's Law to apply?
Flashcards
Law of Combining Volumes
Law of Combining Volumes
States that the volumes of gaseous reactants and products, measured under the same conditions of temperature and pressure, are always whole number ratios.
Avogadro's Law
Avogadro's Law
A law that explains the relationship between the volume of a gas and the number of moles of the gas. It states that the volume of a gas at constant temperature and pressure is directly proportional to the number of moles.
Molar Volume
Molar Volume
At standard temperature and pressure (STP), one mole of any ideal gas occupies a volume of 22.41 liters.
Avogadro's Hypothesis
Avogadro's Hypothesis
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Pressure and Volume Relationship
Pressure and Volume Relationship
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Mathematical Expression of Avogadro's Law
Mathematical Expression of Avogadro's Law
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Kinetic Molecular Theory (KMT)
Kinetic Molecular Theory (KMT)
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Equilibrium
Equilibrium
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Study Notes
Avogadro's Law and Molar Volume
- Avogadro's Law proposes that equal volumes of gases, at the same temperature and pressure, contain the same number of particles.
- Gay-Lussac's Law of Combining Volumes states that the volumes of gaseous reactants and products, measured under the same conditions of temperature and pressure, are always whole number ratios.
- Avogadro's hypothesis explained Gay-Lussac's observations. This hypothesis was initially met with skepticism, but eventually gained acceptance.
- The volume of a gas is directly proportional to the number of moles (n) of the gas, as long as the temperature and pressure are held constant. This relationship is expressed as V ∝ n.
Molar Volume
- The molar volume (v) is the volume occupied by one mole of a gas.
- At standard temperature and pressure (STP), the molar volume is 22.4 L/mol.
- At standard ambient temperature and pressure (SATP), the molar volume is 24.8 L/mol.
- These molar volumes are similar for all gases.
- Molar volume is a conversion factor that can be used for conversions between moles of a gas and its volume when conditions are standard.
Mathematical Expression of Avogadro's Law
- Under constant temperature and pressure, the ratio of the initial volume (V₁) to the number of moles (n₁) is equal to the ratio of the final volume (V₂) to the number of moles (n₂). This is expressed as: n₁/V₁ = n₂/V₂.
Examples
- Examples of calculations are provided demonstrating how to use the molar volume constant to convert moles to volume or volume to moles under standard conditions.
- Example problems show how to use ratios and conversion factors to solve gas law problems.
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