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If a gas is heated while kept in a container with a fixed volume, which of the following will most likely happen according to the ideal gas law?
If a gas is heated while kept in a container with a fixed volume, which of the following will most likely happen according to the ideal gas law?
- The amount of gas (moles) will increase.
- The density of the gas will decrease.
- The pressure of the gas will decrease.
- The pressure of the gas will increase. (correct)
A container of gas has a volume of 10.0 L at a pressure of 2.0 atm and a temperature of 300 K. If the pressure is increased to 4.0 atm while keeping the volume constant, what will the new temperature be, assuming ideal gas behavior?
A container of gas has a volume of 10.0 L at a pressure of 2.0 atm and a temperature of 300 K. If the pressure is increased to 4.0 atm while keeping the volume constant, what will the new temperature be, assuming ideal gas behavior?
- 600 K (correct)
- 150 K
- 450 K
- 300 K
Which of the following statements accurately describes the relationship between the variables in the ideal gas law?
Which of the following statements accurately describes the relationship between the variables in the ideal gas law?
- Temperature is inversely proportional to the number of moles at constant pressure and volume.
- Volume is directly proportional to the number of moles at constant pressure and temperature. (correct)
- Pressure is inversely proportional to temperature at constant volume and moles.
- Pressure is directly proportional to volume at constant temperature and moles.
A gas sample occupies 5.0 L at standard temperature and pressure (STP). If the amount of gas is doubled, what will the new volume be, assuming the temperature and pressure remain constant?
A gas sample occupies 5.0 L at standard temperature and pressure (STP). If the amount of gas is doubled, what will the new volume be, assuming the temperature and pressure remain constant?
What is the impact on the volume of a gas if the number of moles is halved and the absolute temperature is doubled, while the pressure remains constant?
What is the impact on the volume of a gas if the number of moles is halved and the absolute temperature is doubled, while the pressure remains constant?
A balloon contains 0.1 moles of helium gas at 27°C and 1 atm pressure. If 0.2 moles of additional helium gas are added and the temperature is increased to 127°C, what is the ratio of the new volume to the original volume?
A balloon contains 0.1 moles of helium gas at 27°C and 1 atm pressure. If 0.2 moles of additional helium gas are added and the temperature is increased to 127°C, what is the ratio of the new volume to the original volume?
If you have two identical containers, one with hydrogen gas (H2) and the other with oxygen gas (O2), both at the same temperature and pressure, which container has more molecules?
If you have two identical containers, one with hydrogen gas (H2) and the other with oxygen gas (O2), both at the same temperature and pressure, which container has more molecules?
Under what conditions does the behavior of real gases deviate most significantly from the ideal gas law?
Under what conditions does the behavior of real gases deviate most significantly from the ideal gas law?
A gas occupies a volume of 22.4 L at STP. How many moles of gas are present?
A gas occupies a volume of 22.4 L at STP. How many moles of gas are present?
A closed container holds a gas at a constant volume. If the temperature of the gas is increased from 20°C to 40°C, how will the pressure change?
A closed container holds a gas at a constant volume. If the temperature of the gas is increased from 20°C to 40°C, how will the pressure change?
What is the density of methane gas (CH4) at 27°C and 2 atm pressure, given that the molar mass of methane is 16.04 g/mol?
What is the density of methane gas (CH4) at 27°C and 2 atm pressure, given that the molar mass of methane is 16.04 g/mol?
A container holds 4 grams of helium gas at a certain temperature and pressure. If 4 grams of hydrogen gas are added to the same container, without changing the temperature or volume, how does the pressure change? (Molar mass of He = 4 g/mol, H2 = 2 g/mol)
A container holds 4 grams of helium gas at a certain temperature and pressure. If 4 grams of hydrogen gas are added to the same container, without changing the temperature or volume, how does the pressure change? (Molar mass of He = 4 g/mol, H2 = 2 g/mol)
Which of the following changes would cause the volume of a gas to decrease, assuming all other variables remain constant?
Which of the following changes would cause the volume of a gas to decrease, assuming all other variables remain constant?
If the pressure of a gas is doubled and the volume is halved, while the number of moles remains constant, what happens to the temperature?
If the pressure of a gas is doubled and the volume is halved, while the number of moles remains constant, what happens to the temperature?
What is the pressure exerted by 32 grams of oxygen gas (O2) in a 10-liter container at 27°C? (Molar mass of O2 = 32 g/mol)
What is the pressure exerted by 32 grams of oxygen gas (O2) in a 10-liter container at 27°C? (Molar mass of O2 = 32 g/mol)
A sample of nitrogen gas has a volume of 250 mL at 27°C. If the temperature is increased to 77°C, what is the new volume, assuming the pressure and amount of gas remain constant?
A sample of nitrogen gas has a volume of 250 mL at 27°C. If the temperature is increased to 77°C, what is the new volume, assuming the pressure and amount of gas remain constant?
A gas at 2 atm pressure and 273 K occupies a volume of 10 L. If the pressure is reduced to 1 atm and the temperature is increased to 546 K, what is the new volume?
A gas at 2 atm pressure and 273 K occupies a volume of 10 L. If the pressure is reduced to 1 atm and the temperature is increased to 546 K, what is the new volume?
Which of the following units is the correct unit for the universal gas constant (R) when pressure is in atmospheres, volume is in liters, the amount of substance is in moles, and temperature is in Kelvin?
Which of the following units is the correct unit for the universal gas constant (R) when pressure is in atmospheres, volume is in liters, the amount of substance is in moles, and temperature is in Kelvin?
A container holds a mixture of nitrogen and oxygen gas. If the total pressure in the container is 3 atm and the partial pressure of nitrogen is 1 atm, what is the partial pressure of oxygen?
A container holds a mixture of nitrogen and oxygen gas. If the total pressure in the container is 3 atm and the partial pressure of nitrogen is 1 atm, what is the partial pressure of oxygen?
A 5.0 L sealed container at 27°C containsargon gas at a pressure of 1 atm. If 3 grams of argon gas are added to the container, what is the new pressure inside the container, assuming the temperature remains constant? (Molar mass of Ar = 40 g/mol)
A 5.0 L sealed container at 27°C containsargon gas at a pressure of 1 atm. If 3 grams of argon gas are added to the container, what is the new pressure inside the container, assuming the temperature remains constant? (Molar mass of Ar = 40 g/mol)
If the number of moles and the temperature of a gas are both doubled, while the volume remains constant, what happens to the pressure according to the ideal gas law?
If the number of moles and the temperature of a gas are both doubled, while the volume remains constant, what happens to the pressure according to the ideal gas law?
A gas is in a container with a movable piston. Initially, the gas occupies a volume of 5 L at a pressure of 2 atm. If the pressure is increased to 4 atm while keeping the temperature constant, what is the new volume?
A gas is in a container with a movable piston. Initially, the gas occupies a volume of 5 L at a pressure of 2 atm. If the pressure is increased to 4 atm while keeping the temperature constant, what is the new volume?
Which of the following conditions would result in the highest pressure for a fixed amount of gas in a container of fixed volume?
Which of the following conditions would result in the highest pressure for a fixed amount of gas in a container of fixed volume?
A container holds 2 moles of gas A and 3 moles of gas B. If the total pressure is 10 atm, what is the partial pressure of gas A?
A container holds 2 moles of gas A and 3 moles of gas B. If the total pressure is 10 atm, what is the partial pressure of gas A?
If you want to calculate the number of moles of a gas using the ideal gas law, what is the correct formula?
If you want to calculate the number of moles of a gas using the ideal gas law, what is the correct formula?
At standard temperature and pressure (STP), 1 mole of an ideal gas occupies 22.4 L. What volume would 0.25 moles of an ideal gas occupy at twice the standard pressure and the same temperature?
At standard temperature and pressure (STP), 1 mole of an ideal gas occupies 22.4 L. What volume would 0.25 moles of an ideal gas occupy at twice the standard pressure and the same temperature?
A container of fixed volume holds a gas at a certain pressure and temperature. If the gas is heated, what happens to the density of the gas inside the container?
A container of fixed volume holds a gas at a certain pressure and temperature. If the gas is heated, what happens to the density of the gas inside the container?
If you have two gases, A and B, in separate containers of equal volume, both at the same temperature, but gas A has twice the pressure of gas B, which gas has more moles?
If you have two gases, A and B, in separate containers of equal volume, both at the same temperature, but gas A has twice the pressure of gas B, which gas has more moles?
Which of the following best describes how the ideal gas law can be used to determine gas density?
Which of the following best describes how the ideal gas law can be used to determine gas density?
A container has 24 grams of carbon dioxide (CO2) gas at 300 K. Calculate the pressure if the volume of the container is 10 L. (Molar mass of CO2 = 44 g/mol).
A container has 24 grams of carbon dioxide (CO2) gas at 300 K. Calculate the pressure if the volume of the container is 10 L. (Molar mass of CO2 = 44 g/mol).
If the temperature of a gas in a closed container is increased from 27°C to 227°C, by what factor does the pressure increase?
If the temperature of a gas in a closed container is increased from 27°C to 227°C, by what factor does the pressure increase?
What is the volume occupied by 10 grams of hydrogen gas (H2) at a pressure of 2 atm and a temperature of 300 K? (Molar mass of H2 = 2 g/mol)
What is the volume occupied by 10 grams of hydrogen gas (H2) at a pressure of 2 atm and a temperature of 300 K? (Molar mass of H2 = 2 g/mol)
A gas occupies a volume of 10 L at 27°C and 1 atm. If the number of moles is doubled and the temperature is increased to 127°C, what is the new pressure?
A gas occupies a volume of 10 L at 27°C and 1 atm. If the number of moles is doubled and the temperature is increased to 127°C, what is the new pressure?
Which of the following is the correct value and units for the Ideal Gas Constant, R, when using atmospheres for pressure, liters for volume, moles for the amount of gas, and kelvins for temperature?
Which of the following is the correct value and units for the Ideal Gas Constant, R, when using atmospheres for pressure, liters for volume, moles for the amount of gas, and kelvins for temperature?
A balloon contains 4 g of Helium and 16 g of Oxygen at a certain temperature. If the total pressure inside the balloon is 3 atm, what is the partial pressure of Oxygen?
A balloon contains 4 g of Helium and 16 g of Oxygen at a certain temperature. If the total pressure inside the balloon is 3 atm, what is the partial pressure of Oxygen?
A container of gas has a density of 2 g/L at a pressure of 1 atm and a temperature of 300 K. What is the molar mass of the gas?
A container of gas has a density of 2 g/L at a pressure of 1 atm and a temperature of 300 K. What is the molar mass of the gas?
A sample of gas has a volume of 5 liters at a pressure of 2 atm. If the amount of gas is tripled and the temperature is kept constant, what is the new volume if the pressure is also tripled?
A sample of gas has a volume of 5 liters at a pressure of 2 atm. If the amount of gas is tripled and the temperature is kept constant, what is the new volume if the pressure is also tripled?
A container with a volume of 22.4 L holds 2 moles of nitrogen gas at 273 K. What is the pressure in the container?
A container with a volume of 22.4 L holds 2 moles of nitrogen gas at 273 K. What is the pressure in the container?
A gas is compressed to half of its original volume and its temperature is doubled. What happens to its number of moles?
A gas is compressed to half of its original volume and its temperature is doubled. What happens to its number of moles?
Helium gas is in a sealed container, and you observe that if you increase the temperature you also increase the pressure. Which of the following statements is true?
Helium gas is in a sealed container, and you observe that if you increase the temperature you also increase the pressure. Which of the following statements is true?
Flashcards
Ideal Gas Law
Ideal Gas Law
PV = nRT, relates pressure, volume, moles, and temperature of an ideal gas.
Pressure Unit in Ideal Gas Law
Pressure Unit in Ideal Gas Law
Pressure must be in atmospheres (atm) for the ideal gas law.
Volume Unit in Ideal Gas Law
Volume Unit in Ideal Gas Law
Volume must be in liters (L) for the ideal gas law.
Temperature Unit in Ideal Gas Law
Temperature Unit in Ideal Gas Law
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n in PV=nRT
n in PV=nRT
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Value of R
Value of R
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Density Calculation Formula (Ideal Gas Law)
Density Calculation Formula (Ideal Gas Law)
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What is PV = nRT?
What is PV = nRT?
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What is the universal gas constant (R)?
What is the universal gas constant (R)?
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Celsius to Kelvin conversion
Celsius to Kelvin conversion
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How to calculate moles?
How to calculate moles?
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O2 Molar Mass
O2 Molar Mass
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Study Notes
Ideal Gas Law
- PV = nRT mathematically relates pressure, volume, number of moles, and temperature of a gas.
- P represents pressure; it must be in atmospheres (atm).
- V represents volume; it must be in liters (L).
- n represents the number of moles of gas.
- T represents the temperature of the gas; it must be in Kelvins (K).
- Pressure, volume, temperature, and quantity (moles) are the four key properties of gases.
- R is the universal gas constant that balances the equation.
- R = 0.0821 L atm / (mol K)
- For greater precision, R may be expressed as 0.08206 L atm / (mol K).
- Units for R are liter atmospheres per mole Kelvin.
- For the constant to work, other units must be in Kelvins, moles, liters, and atmospheres.
Example Problem 1
- A rigid steel container has a volume of 20.0 liters and holds nitrogen gas at 200 atmospheres at 27 degrees Celsius.
- The problem seeks the number of moles of nitrogen gas in the cylinder.
- Solution:
- P = 200 atm
- V = 20.0 L
- n = unknown
- R = 0.0821 L atm / (mol K)
- T = 27°C = 300 K
- 200 atm * 20.0 L = n * 0.0821 L atm / (mol K) * 300 K
- n ≈ 162 moles
Example Problem 2
- The problem is to find the volume of 12.0 grams of oxygen gas (O2) at 25 degrees Celsius and 0.520 atmospheres.
- P = 0.520 atm
- V = unknown
- Convert grams of O2 to moles:
-
- 0 g O2 / 32.00 g/mol = 0.375 moles O2
-
- n = 0.375 moles
- R = 0.0821 L atm / (mol K)
- T = 25°C = 298 K
-
- 520 atm * V = 0.375 moles * 0.0821 L atm / (mol K) * 298 K
- V ≈ 17.6 liters
Density Calculation
- Problem: Calculate the density of oxygen gas (O2) in grams per liter at 25 degrees Celsius and 1.00 atmospheres.
- Density is found by incorporating grams into the problem to get grams/liter.
- Moles (n) = grams / molar mass
- Substitute grams / molar mass for n in the ideal gas law: PV = (grams / molar mass)RT
- grams/volume = (Pressure * molar mass) / (R * T) after rearranging the equation to solve for grams/volume (density).
- Solution:
- Pressure = 1.00 atm
- Molar mass of O2 = 32.00 g/mol
- R = 0.0821 L atm / (mol K)
- T = 25°C = 298 K
- Density = (1.00 atm * 32.00 g/mol) / (0.0821 L atm / (mol K) * 298 K)
- Density ≈ 1.31 grams per liter
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