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Questions and Answers
What happens to the volume of a gas when pressure increases?
What happens to the volume of a gas when pressure increases?
- It remains constant
- It changes slightly
- It decreases significantly (correct)
- It increases significantly
Under standard conditions of temperature and pressure (STP), what is the standard molar volume of one mole of gas?
Under standard conditions of temperature and pressure (STP), what is the standard molar volume of one mole of gas?
- 11.414 liters
- 30.414 liters
- 22.414 liters (correct)
- 10.414 liters
Which law states that the volume of a gas is directly proportional to its temperature when pressure is held constant?
Which law states that the volume of a gas is directly proportional to its temperature when pressure is held constant?
- Charles’s Law (correct)
- Ideal Gas Law
- Boyle’s Law
- Avogadro’s Law
What is Avogadro's number that represents the number of particles in one mole of a substance?
What is Avogadro's number that represents the number of particles in one mole of a substance?
What is a property of gases that distinguishes them from liquids and solids?
What is a property of gases that distinguishes them from liquids and solids?
What is the relationship between the number of particles and the volume of gas at the same temperature and pressure according to Avogadro's Law?
What is the relationship between the number of particles and the volume of gas at the same temperature and pressure according to Avogadro's Law?
At what temperature is standard temperature defined in Celsius?
At what temperature is standard temperature defined in Celsius?
Which of the following statements about gas viscosity is true?
Which of the following statements about gas viscosity is true?
What happens to gases at low temperatures and high pressures?
What happens to gases at low temperatures and high pressures?
Which equation represents the relationship between real and ideal pressures for gases?
Which equation represents the relationship between real and ideal pressures for gases?
When calculating the pressure in a flask using the ideal gas law, which value represents the number of moles of gas if there is 1 mole of methane?
When calculating the pressure in a flask using the ideal gas law, which value represents the number of moles of gas if there is 1 mole of methane?
In the Van der Waals equation, what does the 'a' parameter account for?
In the Van der Waals equation, what does the 'a' parameter account for?
For the ideal gas behavior of methane at 25°C and 244.6 mL, what is the pressure calculated in atm?
For the ideal gas behavior of methane at 25°C and 244.6 mL, what is the pressure calculated in atm?
What is the effect of significant intermolecular interactions on gas behavior?
What is the effect of significant intermolecular interactions on gas behavior?
Using the Van der Waals equation, if 'b' is the molar volume of the gas molecules, what must we subtract from the volume in the equation?
Using the Van der Waals equation, if 'b' is the molar volume of the gas molecules, what must we subtract from the volume in the equation?
What are the conditions under which most gases exhibit nearly ideal behavior?
What are the conditions under which most gases exhibit nearly ideal behavior?
What is the correct relationship defined by Avogadro's Law?
What is the correct relationship defined by Avogadro's Law?
What is the appropriate value of the universal gas constant (R) in terms of J/(mol·K)?
What is the appropriate value of the universal gas constant (R) in terms of J/(mol·K)?
According to Dalton's law of partial pressures, how is the total pressure of a gas mixture calculated?
According to Dalton's law of partial pressures, how is the total pressure of a gas mixture calculated?
In the ideal gas law, what does the variable 'n' represent?
In the ideal gas law, what does the variable 'n' represent?
Using the combined gas law, if the pressure of a gas is constant, which formula can be used to find the new amount of gas remaining when heated?
Using the combined gas law, if the pressure of a gas is constant, which formula can be used to find the new amount of gas remaining when heated?
When a gas is heated at constant volume, how does its pressure change according to Charles's Law?
When a gas is heated at constant volume, how does its pressure change according to Charles's Law?
What is calculated using the values of total pressure and mole fractions in a gas mixture?
What is calculated using the values of total pressure and mole fractions in a gas mixture?
What happens to the volume of an ideal gas if the temperature is doubled while keeping the pressure constant?
What happens to the volume of an ideal gas if the temperature is doubled while keeping the pressure constant?
Flashcards
Gas Volume Change with Pressure
Gas Volume Change with Pressure
The volume of a gas is significantly affected by changes in pressure.
Gas Volume Change with Temperature
Gas Volume Change with Temperature
The volume of a gas is significantly affected by changes in temperature.
Gas Viscosity
Gas Viscosity
Gases have very low viscosity, meaning they flow easily.
Gas Density
Gas Density
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Gas Miscibility
Gas Miscibility
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Avogadro's Law
Avogadro's Law
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Standard Molar Volume
Standard Molar Volume
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Mole (chemistry)
Mole (chemistry)
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Ideal Gas Law
Ideal Gas Law
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Avogadro's Law
Avogadro's Law
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Boyle's Law
Boyle's Law
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Charles' Law
Charles' Law
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Partial Pressure
Partial Pressure
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Dalton's Law of Partial Pressures
Dalton's Law of Partial Pressures
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Gas Density
Gas Density
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Gas Molar Mass
Gas Molar Mass
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Ideal Gas Behavior
Ideal Gas Behavior
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Real Gas Deviation
Real Gas Deviation
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Intermolecular Interaction
Intermolecular Interaction
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Van der Waals Equation
Van der Waals Equation
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Van der Waals Constants(a)
Van der Waals Constants(a)
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Van der Waals Constants(b)
Van der Waals Constants(b)
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Ideal Gas Law
Ideal Gas Law
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Partial Pressure of Oxygen
Partial Pressure of Oxygen
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Study Notes
Gases
- Gases have properties that distinguish them from liquids and solids.
- Gas volume changes significantly with pressure.
- Gas volume changes significantly with temperature.
- Gases have relatively low viscosity and flow rapidly. This is because of weak interactions between gas molecules.
- Most gases have relatively low densities under normal conditions. A small amount of gas can occupy a large volume.
- Gases are miscible (mix in any proportion) and have no phase boundaries.
- Gaseous samples can be described by four variables.
- Volume (V) in liters (L)
- Amount (n) in moles
- Temperature (T) in Kelvin (K)
- Pressure (P) in atmospheres (atm)
Gas Laws
-
Boyle's Law: PV = constant (at constant temperature and amount of gas).
- As pressure increases, volume decreases.
-
Charles's Law: V/T = constant (at constant pressure and amount of gas).
- As temperature increases, volume increases.
-
Avogadro's Law: V/n = constant (at constant temperature and pressure).
- The volumes of gases at the same temperature and pressure contain the same number of particles.
- One mole of any gas at STP occupies the same volume (22.414 liters).
- STP: Standard Temperature and Pressure (0°C, 1 atm)
Ideal Gas Law
- PV = nRT
- P = Pressure
- V = Volume
- n = Number of moles
- R = Ideal Gas Constant
- T = Temperature
- R has values depending on the units used for P, V, n, and T.
Gas Density and Gas Molar Mass
-
Gas density is determined by: d = m/V = PM/RT
- d = density
- m = mass
- V = volume
- P = pressure
- R = ideal gas constant
- T = temperature
- M = molar mass
-
The molar mass of a gas is determined by: M = mRT/PV
Dalton's Law of Partial Pressures
- The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases.
-
PTotal = P1 + P2 + P3... where P1, P2, etc. are the partial pressures of the individual gases.
-
The partial pressure of each gas is proportional to its mole fraction, x.
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P1 = x1 Ptotal
-
Deviation of Real Gases from Ideal Behavior
- Real gases do not always follow the ideal gas law precisely, especially at high pressure and low temperature.
- Intermolecular forces and the volume of the gas molecules themselves affect the behavior of real gases.
- Corrections are made to the ideal gas law (Van der Waals Equation) to account for these factors.
- Van der Waals Equation is used to correct for intermolecular attractions and the volume of gas molecules.
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