Empirical Properties of Gases

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Questions and Answers

Which statement best describes the behavior of gases?

  • Gases fill and take the shape of their container, having neither a fixed shape nor volume. (correct)
  • Gases maintain a fixed shape and volume.
  • Gases have a definite shape but can be compressed into smaller volumes.
  • Gases have a definite volume but take the shape of their container.

Gases typically have the highest density compared to solids and liquids.

False (B)

Gases mix completely and uniformly with other gases when __________.

confined

What four variables define the state of a gaseous substance?

<p>Chemical amount, pressure, volume, and temperature.</p> Signup and view all the answers

What does 1 atm equal in kilopascals (kPa)?

<p>101.325 kPa (C)</p> Signup and view all the answers

In chemistry, pressure is usually expressed in Pascals (Pa).

<p>False (B)</p> Signup and view all the answers

In the context of gases, volume is the __________ occupied by the gas and is measured in __________.

<p>space, litres</p> Signup and view all the answers

What is the standard temperature used in gas law calculations?

<p>Kelvin (A)</p> Signup and view all the answers

According to Boyle's Law, if the pressure of a gas increases, the volume also increases, assuming temperature and chemical amount remain constant.

<p>False (B)</p> Signup and view all the answers

Boyle's Law states that pressure and volume are __________ proportional.

<p>inversely</p> Signup and view all the answers

Which law describes the relationship between temperature and volume of a gas at constant pressure?

<p>Charles's Law (C)</p> Signup and view all the answers

In Charles's Law, temperature can be measured in Celsius for accurate calculations.

<p>False (B)</p> Signup and view all the answers

Match each gas law with its correct mathematical expression, where P is pressure, V is volume, T is temperature, and k is a constant:

<p>Boyle's Law = $P_1V_1 = P_2V_2$ Charles's Law = $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ Combined Gas Law = $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$</p> Signup and view all the answers

The Combined Gas Law states that the __________ of pressure and volume is proportional to __________.

<p>product, temperature</p> Signup and view all the answers

Which gas law describes the relationship between pressure and temperature when volume is constant?

<p>Gay-Lussac's Law (D)</p> Signup and view all the answers

According to the Kinetic Molecular Theory (KMT), gas particles are considered to have significant attractive forces between them.

<p>False (B)</p> Signup and view all the answers

Explain how Kinetic Molecular Theory (KMT) describes the compressibility of gases.

<p>Compressibility is explained by the large spaces between gas particles, allowing them to be forced closer together under pressure.</p> Signup and view all the answers

According to KMT, the kinetic energy of gas particles is __________ to temperature.

<p>proportional</p> Signup and view all the answers

What happens to the collision frequency of gas particles in a container when the volume of the container is reduced, according to KMT?

<p>Collision frequency increases. (D)</p> Signup and view all the answers

Avogadro's Theory states that at the same temperature and pressure, equal volumes of gases contain equal numbers of atoms.

<p>False (B)</p> Signup and view all the answers

Explain the law of combining volumes.

<p>When temperature and pressure are constant, the volumes of gaseous reactants and products are in simple, whole-number ratios.</p> Signup and view all the answers

Molar volume refers to the _________ that one __________ of a gas occupies at a specific temperature and pressure.

<p>volume, mole</p> Signup and view all the answers

What is the molar volume of a gas at SATP (Standard Ambient Temperature and Pressure)?

<p>24.8 L/mol (A)</p> Signup and view all the answers

The molar volume of all gases is the same regardless of temperature and pressure conditions.

<p>False (B)</p> Signup and view all the answers

Describe how molar volume is used as a conversion factor in gas stoichiometry.

<p>Molar volume converts chemical amount (moles) of gas to its volume and vice versa, facilitating quantitative analysis in chemical reactions.</p> Signup and view all the answers

An ideal gas is a __________ gas that perfectly obeys all the gas laws under __________ conditions.

<p>hypothetical, all</p> Signup and view all the answers

Which assumption is made about ideal gases according to the Kinetic Molecular Theory (KMT)?

<p>Gas molecules are far apart relative to their size. (B)</p> Signup and view all the answers

At very high pressures, the size of gas particles becomes negligible, leading gases to behave more ideally.

<p>False (B)</p> Signup and view all the answers

Describe the conditions under which real gases behave most like ideal gases.

<p>Real gases behave most ideally under relatively low pressure and high temperature.</p> Signup and view all the answers

The Ideal Gas Law is represented mathematically as PV = __________, where n is the chemical amount, and R is the __________.

<p>nRT, ideal gas constant</p> Signup and view all the answers

What is the standard value of the ideal gas constant (R) when pressure is in kPa and volume is in liters?

<p>8.314 kPa L / (mol K) (A)</p> Signup and view all the answers

Dalton's Law of Partial Pressures applies only to gases that do not react with each other.

<p>True (A)</p> Signup and view all the answers

State Dalton's Law of Partial Pressures.

<p>Dalton's Law states that the total pressure exerted by a mixture of gases is the sum of the partial pressures of each gas in the mixture.</p> Signup and view all the answers

According to Dalton's Law, the partial pressure of each gas in a mixture is the __________ exerted by the gas if it occupied the container __________.

<p>pressure, alone</p> Signup and view all the answers

Which of the following is an application of stoichiometric principles to gaseous reactions?

<p>Analyzing the quantity of gas involved in a chemical reaction (A)</p> Signup and view all the answers

When using gas stoichiometry, it is unnecessary to balance the chemical reaction equation.

<p>False (B)</p> Signup and view all the answers

Explain the role of coefficients in a balanced chemical reaction equation for gas stoichiometry.

<p>Coefficients indicate the mole ratios of reactants and products, enabling calculations to predict gas quantities involved in the reaction.</p> Signup and view all the answers

When conditions are not at STP or SATP, or when reactants or products are not gases, the __________ must be used to complete calculations in gas stoichiometry.

<p>Ideal Gas Law</p> Signup and view all the answers

A gas occupies 10.0 L at 150°C and 150 kPa. What information is necessary according to the Ideal Gas Law to calculate the mass of calcium carbonate (CaCO3) needed to produce this gas?

<p>The balanced chemical reaction equation and molar mass (B)</p> Signup and view all the answers

A balloon contains helium gas at 20 °C with a volume of 7.50 L at 100 kPa. The balloon rises to an altitude where the temperature is -36 °C and the outside pressure is 28 kPa. Assuming the balloon expands freely and no gas escapes, calculate the new volume of the balloon.

<p>22 L (C)</p> Signup and view all the answers

A rigid 3.0L container holds N2 gas at 20.0°C and 3.00 atm. What will be the pressure if the container is placed in a 50.0°C oven, assuming the volume remains constant?

<p>3.30 atm (D)</p> Signup and view all the answers

If Mrs. Litzenberger fills her tires to 34 psi, what is this pressure in atm and kPa?

<p>2.3 atm , 232 kPa (C)</p> Signup and view all the answers

Flashcards

Gas properties

Gases fill and take the shape and volume of their containers.

Gas diffusion

Gases move spontaneously throughout space.

Compressibility

Gases are easily squeezed into smaller volumes.

Gas mixing

Gases mix completely and uniformly when confined.

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Gas pressure

Gases exert a force on their surroundings.

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Pressure definition

The force exerted per unit area.

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Pressure measurement

Force per unit area; measured in Pascals (Pa).

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Boyle's Law

As pressure increases, volume decreases; temperature is constant.

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Charles's Law

As temperature increases, volume increases; pressure is constant.

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Combined Gas Law

The product of pressure & volume is proportional to temperature.

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Gay-Lussac's Law

Pressure is directly proportional to temperature; volume is constant.

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Kinetic Energy

Kinetic energy of gas particles is proportional to temperature.

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Avogadro's Theory

At same temperature & pressure, gases contain equal volumes of molecules.

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Molar Volume

Mass of a substance required to produce one mole of gas.

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Ideal Gas

Hypothetical gas that perfectly obeys all gas laws under all conditions.

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Ideal Gas Constant

A constant relating the properties of ideal gases.

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Real Gases at high pressures

At high pressures, molecules are forced together so size of gas particles their size matters is negligible

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Partial Pressure Definition

The pressure exerted by an individual gas in a mixture.

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Dalton's Law

The total pressure of a mixture of gases is the sum of the partial pressures.

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Stoichiometry

Analyze quantities of reactants or products, using mole ratios and balanced chemical equations.

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Gas Stoichiometry

Predicts or analyzes the quantity of gas involved in chemical reactions.

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Study Notes

Empirical Properties of Gases

  • Gases fill and take the shape of their containers
  • Gases have neither a shape nor volume of their own
  • Gases diffuse and/or move spontaneously throughout space
  • Most gases are colourless and odourless
  • Gases are highly compressible; when pressure increases in a gas, its volume decreases, and vice-versa
  • If temperature of gas ↑ then the volume of gas ↑
  • If pressure of gas ↑ then the volume of gas ↓
  • Gases have the lowest density of all states of matter
  • Gases have the weakest intermolecular forces of all states of matter
  • Gases mix completely and uniformly with other gases when confined in the same space if no chemical reaction occurs
  • Gases exert pressure on its surroundings

Defining State of a Gaseous Substance

  • The state is defined by four variables: chemical amount, pressure, volume, and temperature
  • Chemical amount is measured in moles
  • Pressure (P) is force per unit area, measured in Pascals(Pa)
  • 1 kPa = 1000 Pa
  • 1 kPa = 1000 N/m²
  • 1 atm = 101,325 kPa = 760 mm Hg (millimeters of mercury)
  • 1 atm is also known as 1 atmosphere
  • 14.7 psi = 1.01 bar
  • Pressure in chemistry is usually expressed in atm, using dimensional analysis (ratios) to convert

Volume

  • Volume (V) is the space occupied by a gas
  • Volume is measured in Litres (L)

Temperature

  • Temperature (T) of gases measured in Kelvin (K)
  • To convert from Celsius to Kelvin: T(K) = T(°C) + 273

Standard Conditions

  • Scientists define standard conditions:
    • Standard Temperature and Pressure (STP): 0°C (273 K) and 1 atm (101kPa)
    • Standard Ambient Temperature and Pressure (SATP): 25°C = 298K

Boyle's Law

  • The law describes the relationship between pressure and volume
  • As pressure of a gas increases, volume decreases, inversely proportional
  • Temperature and chemical amount must remain constant
  • Boyle's Law is written mathematically as P₁V₁ = P₂V₂

Charles' Law

  • The law describes the relationship between temperature and volume
  • As temperature increases, volume of a gas also increases if pressure and molarity are kept constant
  • Charles' Law can be written mathematically as V₁/T₁ = V₂/T₂
  • The temperature (T) must always be in Kelvin (K)
  • Relationship between volume and temperature is directly proportional

Combined Gas Law

  • The combined gas law relates pressure, volume, and temperature
  • Product of pressure and volume of a gas is proportional to temperature, (molar amount is constant)
  • Combined Gas Law: P₁V₁/T₁ = P₂V₂/T₂

Kinetic Molecular Theory of Gases

  • The kinetic energy of gas particles is proportional to temperature
  • As temperature increases, so does the kinetic energy of the gas particles
  • Explains why gases are highly compressible because gas particles are far apart
  • It's possible to force the particles closer together when pressure is applied
  • Gas pressure is the total force of the collisions of gas particles distributed over an area of that container
  • Boyle's Law: If the volume of the container is reduced, gas particles travel shorter distances to collide with their container, therefore they collide more frequently, leading to an increased pressure on the container
  • Charles' Law: An increase in temperature represents an average kinetic energy

Law of Combining Volumes

  • When temperature and pressure are constant, the volume of gaseous reactants and products are in simple whole number ratios
  • Avogadro's Theory states that at the same temperature and pressure, equal volumes of gases contain equal numbers of molecules

Molar Volume

  • Molar Volume refers to the volume one mole of gas occupies at a specific temperature and pressure
  • Molar volume is the conversion factor to convert chemical amount of gas to volume
  • Volume (V) = amount (n) x Molar Volume (VM)
  • 24.8 L/mol = VSATP and 22.4 L/mol at VSTP

Ideal Gas Law

  • The law describes a hypothetical gas that perfectly obeys all the gas laws under all conditions
  • Gases are far apart relative to their size
  • At high pressures, molecules are forced together so the size of particles and their size matters is negligible
  • Constant, random, straight-line motion
  • Collisions of gas particles are elastic and no NRG is lost
  • At relatively low pressure and high temperature (STP and SATP), real gases behave like ideal gases
  • Ideal Gas Law: PV = nRT.
  • R (the ideal gas constant) = 8.314 kPa

Dalton's Law of Partial Pressure

  • Partial Pressure is the pressure exerted by an individual gas in a mixture
  • Dalton's Law of Partial Pressures- the total pressure of a mixture is the sum of the partial pressures of each of the gases in the mixture

Gas Stoichiometry

  • Gas Stoichiometry predicts or analyzes the quantity of gas involved in a chemical reaction
  • Molar volume and molar mass can be used to convert between volume and mass

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