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Questions and Answers
Why do we assume gas molecules have zero volume on their own?
Why do we assume gas molecules have zero volume on their own?
To prevent larger errors in volume calculations when the space around the gas is small.
A lower volume of container results in a _________ which results in inaccurate volume calculations.
A lower volume of container results in a _________ which results in inaccurate volume calculations.
significant difference
Why do we assume there are no intermolecular forces between gas molecules?
Why do we assume there are no intermolecular forces between gas molecules?
To prevent the gas molecules from being closer together, taking less space and pressure.
Why do we assume molecules move in perfectly straight line in ideal gas law?
Why do we assume molecules move in perfectly straight line in ideal gas law?
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A gas with a _______ intermolecular force results in it acting more like an _______.
A gas with a _______ intermolecular force results in it acting more like an _______.
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What is Avogadro's theory?
What is Avogadro's theory?
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What is the formula for Avogadro's theory?
What is the formula for Avogadro's theory?
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What is molar volume?
What is molar volume?
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What is the molar volume of gases at STP?
What is the molar volume of gases at STP?
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What is the molar volume of gases at SATP?
What is the molar volume of gases at SATP?
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What are the variables in the ideal gas law?
What are the variables in the ideal gas law?
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Describe the relationship between PV/T and n.
Describe the relationship between PV/T and n.
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Study Notes
Ideal Gas Assumptions
- Gas molecules are assumed to have zero volume because their size is negligible compared to the container.
- A lower volume of container results in a higher pressure, which can lead to inaccurate volume calculations.
Ideal Gas Behavior
- Gas molecules are assumed to have no intermolecular forces between them, making their behavior ideal.
Molecular Motion
- Molecules are assumed to move in perfectly straight lines in the ideal gas law, which is not true in reality.
Real Gas Behavior
- A gas with stronger intermolecular forces results in it acting more like a real gas, deviating from ideal behavior.
Avogadro's Theory
- Avogadro's theory states that equal volumes of gases at the same temperature and pressure contain an equal number of molecules.
- The formula for Avogadro's theory is V1 / n1 = V2 / n2.
Molar Volume
- Molar volume is the volume occupied by one mole of a gas.
- The molar volume of gases at STP (Standard Temperature and Pressure) is 22.4 L/mol.
- The molar volume of gases at SATP (Standard Ambient Temperature and Pressure) is 24.45 L/mol.
Ideal Gas Law
- The variables in the ideal gas law are P (pressure), V (volume), n (number of moles), R (gas constant), and T (temperature in Kelvin).
- The ideal gas law is PV = nRT.
- The relationship between PV/T and n is constant, meaning that PV/T = nR.
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Description
Test your knowledge on ideal gases, Avogadro's theory, molar volume, and the molar volume of gases at STP. This quiz covers the assumptions of ideal gases, Avogadro's theory formula, and the concept of molar volume.
