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Chemistry Semester 2 > Gas Laws Round 1 > Flashcards

Gas Laws Round 1 Flashcards

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1
Q

What is the general gas equation?

A

PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant, and T = temperature.

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2
Q

Define Boyle’s Law.

A

Boyle’s Law states that at a constant temperature, the pressure of a gas is inversely proportional to its volume (P1V1 = P2V2).

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3
Q

Define Charles’s Law.

A

Charles’s Law states that at constant pressure, the volume of a gas is directly proportional to its temperature (V1/T1 = V2/T2).

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4
Q

What is Avogadro’s Law?

A

Avogadro’s Law states that at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles (V ∝ n).

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5
Q

State Gay-Lussac’s Law.

A

Gay-Lussac’s Law states that at constant volume, the pressure of a gas is directly proportional to its temperature (P1/T1 = P2/T2).

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6
Q

What units are commonly used for pressure in gas law calculations?

A

Atmospheres (atm), millimeters of mercury (mmHg), and Pascals (Pa).

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7
Q

What is the standard temperature and pressure (STP) for gases?

A

0°C (273 K) and 1 atm pressure.

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8
Q

What does the ‘R’ in the ideal gas law stand for?

A

‘R’ is the gas constant, which equals 0.0821 atm·L/(mol·K) when using atm, liters, and Kelvin.

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9
Q

What is partial pressure?

A

The pressure exerted by each individual gas in a mixture.

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10
Q

State Dalton’s Law of Partial Pressures.

A

Dalton’s Law states that the total pressure of a mixture of gases is the sum of the partial pressures of each gas (P_total = P1 + P2 + P3 …).

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11
Q

What is diffusion?

A

The process of gas molecules spreading out to fill the available volume.

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12
Q

Define effusion.

A

Effusion is the process where gas particles escape through a tiny hole into a vacuum.

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13
Q

State Graham’s Law of Effusion.

A

The rate of effusion of a gas is inversely proportional to the square root of its molar mass (Rate1/Rate2 = √(M2/M1)).

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14
Q

How does the molar volume of an ideal gas at STP compare across gases?

A

The molar volume is the same for all ideal gases at STP, approximately 22.4 L.

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15
Q

Define the term ‘ideal gas.’

A

An ideal gas is a hypothetical gas that perfectly follows the gas laws under all conditions.

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16
Q

What assumptions are made about ideal gases?

A

Ideal gases are assumed to have no intermolecular forces and occupy no volume.

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17
Q

What is the kinetic molecular theory?

A

A theory that describes gas behavior in terms of particle motion, collision, and kinetic energy.

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18
Q

What is the relationship between kinetic energy and temperature in gases?

A

The average kinetic energy of gas particles is directly proportional to the absolute temperature.

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19
Q

What is meant by ‘real gases’?

A

Real gases deviate from ideal gas behavior due to intermolecular forces and molecular volume.

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20
Q

Under what conditions do gases deviate most from ideal behavior?

A

At low temperatures and high pressures.

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21
Q

What is the Van der Waals equation?

A

An equation that modifies the ideal gas law to account for intermolecular forces and molecular volume.

22
Q

Why is the ideal gas law considered an approximation?

A

It assumes gases have no interactions and particles occupy no space, which isn’t true for real gases.

23
Q

What is meant by the compressibility of a gas?

A

Compressibility measures how much the volume of a gas decreases under pressure.

24
Q

What is molar mass and how is it used in gas law calculations?

A

Molar mass is the mass of one mole of a substance, used to relate mass to moles in gas calculations.

25
Q

How can you calculate the density of a gas using the ideal gas law?

A

Density (d) = (PM) / (RT), where M is the molar mass.

26
Q

How does temperature affect gas pressure?

A

An increase in temperature increases the kinetic energy and thus increases the pressure of a gas.

27
Q

How does molecular weight affect the speed of gas molecules?

A

Lighter gas molecules move faster than heavier ones at the same temperature.

28
Q

Why do gases have low densities?

A

The particles are widely spaced, occupying a large volume relative to their mass.

29
Q

Explain why gas pressure is caused.

A

Pressure is caused by collisions of gas molecules with the walls of their container.

30
Q

What happens to gas volume if the pressure is doubled while temperature remains constant?

A

The volume is halved (Boyle’s Law).

31
Q

How does the addition of gas molecules affect pressure?

A

Increasing the number of molecules in a fixed volume increases the pressure.

32
Q

What is meant by an elastic collision in the kinetic molecular theory?

A

A collision where no kinetic energy is lost.

33
Q

What is a vacuum?

A

A space with no particles and therefore no pressure.

34
Q

Why do gases expand to fill their container?

A

Gas particles move freely and spread out until they occupy all available space.

35
Q

How does atmospheric pressure change with altitude?

A

Atmospheric pressure decreases with higher altitude.

36
Q

How does a barometer work?

A

A barometer measures atmospheric pressure by balancing mercury in a column against air pressure.

37
Q

What is absolute zero?

A

The theoretical temperature at which all molecular motion stops (0 K or -273.15°C).

38
Q

What happens to gas particles at absolute zero?

A

They have minimum possible kinetic energy.

39
Q

How does increasing temperature affect gas volume?

A

Volume increases if the pressure remains constant (Charles’s Law).

40
Q

How can molar volume be used to find moles of gas?

A

At STP, volume (L) divided by 22.4 L/mol gives moles of gas.

41
Q

What is the relationship between the speed of gas molecules and temperature?

A

As temperature increases, the average speed of gas molecules increases.

42
Q

How does temperature affect the kinetic energy distribution of gas molecules?

A

Higher temperatures broaden the distribution and increase average kinetic energy.

43
Q

Describe the Maxwell-Boltzmann distribution curve.

A

It shows the range of speeds of gas molecules at a given temperature.

44
Q

What is the most probable speed in a Maxwell-Boltzmann distribution?

A

The speed at which the greatest number of molecules move.

45
Q

What is the impact of intermolecular forces on real gas behavior?

A

Intermolecular attractions reduce the pressure exerted by real gases compared to ideal gases.

46
Q

Explain how a gas exerts pressure on the walls of its container.

A

Gas particles collide with the container walls, transferring momentum and creating pressure.

47
Q

In terms of kinetic energy, why does a gas expand when heated?

A

Increased kinetic energy leads to faster-moving particles that spread apart, expanding the volume.

48
Q

How can the ideal gas law be used to calculate molar mass?

A

Molar mass (M) = (dRT) / P, where d is the density of the gas.

49
Q

How does the real gas equation adjust for the volume of gas particles?

A

The Van der Waals equation includes a term for particle volume (b).

50
Q

What happens to the ideal gas behavior at very low temperatures?

A

Ideal gas behavior deviates as particles slow and attractive forces become significant.

51
Q
A

Chemistry Semester 2 (14 decks)

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