Gas Laws Learning Guide 5.1 & 5.2
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Questions and Answers

What happens to the volume of a gas when the pressure increases, according to Boyle's Law?

  • The volume becomes zero.
  • The volume stays the same.
  • The volume increases.
  • The volume decreases. (correct)
  • At standard temperature and pressure (STP), what is the volume occupied by 1 mole of gas?

  • 10.5 L
  • 22.4 L (correct)
  • 12.3 L
  • 15.0 L
  • What is the temperature in Kelvin when the temperature is 25 degrees Celsius?

  • 298.15 K (correct)
  • 310.15 K
  • 300.15 K
  • 273.15 K
  • If a balloon is exposed to heat, what effect does this typically have on the gas inside it?

    <p>The gas expands.</p> Signup and view all the answers

    If a diver's lungs contain 5.82 L of air at a surface pressure of 1 atm, what will the volume be at a depth where the pressure is 1.92 atm?

    <p>3.02 L</p> Signup and view all the answers

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

    <p>Higher temperatures correspond to faster particles.</p> Signup and view all the answers

    What condition causes the pressure of a gas to remain constant according to gas laws?

    <p>Constant amount of gas</p> Signup and view all the answers

    The relationship defined by Avogadro’s Law describes how the volume of a gas is affected by what variable?

    <p>Moles of gas</p> Signup and view all the answers

    What happens to the pressure in the lungs when they expand during inhalation?

    <p>Pressure decreases</p> Signup and view all the answers

    Why is it difficult to compress a sealed soda bottle filled with carbon dioxide and water?

    <p>The air molecules are tightly packed</p> Signup and view all the answers

    How does the pressure change when the plunger of a syringe is pushed down?

    <p>Pressure increases because volume decreases</p> Signup and view all the answers

    What effect does ascending from underwater have on a diver's blood gas solubility?

    <p>Solubility decreases due to reduced pressure</p> Signup and view all the answers

    What is the practical application of Boyle's Law in inflating tires?

    <p>Compressed air increases tire pressure</p> Signup and view all the answers

    What must be considered to use Charles’ Law effectively at constant pressure?

    <p>Volume changes directly with temperature</p> Signup and view all the answers

    Which scenario accurately represents Boyle's Law in action?

    <p>Pushing down on a syringe increases the pressure inside</p> Signup and view all the answers

    What happens to the volume of gas when its temperature is increased at constant pressure?

    <p>Volume increases</p> Signup and view all the answers

    What is the volume of nitrogen at 333 K given an initial volume of 50.0 mL at 298 K?

    <p>55.9 mL</p> Signup and view all the answers

    What is the new volume of a gas if its initial pressure is 2.44 atm, initial volume is 4.01 L, and pressure changes to 1.93 atm?

    <p>3.67 L</p> Signup and view all the answers

    At what pressure will a gas with an initial volume of 88.8 mL and a final volume of 0.663 L achieve equilibrium?

    <p>722 torr</p> Signup and view all the answers

    A balloon that can hold a maximum volume of 2.5 L contains 2.0 L of helium at sea level. If it rises to an altitude where the pressure is 88.144 kPa, will it burst?

    <p>No, it will not burst.</p> Signup and view all the answers

    When the volume of a gas changes from ___ mL to 852 mL, with a temperature change from 315 °C to 452 °C, what is the starting volume?

    <p>410 mL</p> Signup and view all the answers

    According to Avogadro's law, what will be the new volume if 5.00 L of gas is increased from 0.965 mol to 1.80 mol?

    <p>9.09 L</p> Signup and view all the answers

    What relationship does Avogadro’s law describe?

    <p>Volume is directly proportional to the number of moles.</p> Signup and view all the answers

    If the initial volume of a gas raises from 4.01 L to 5.00 L, given a change in pressure from 1.44 atm to what new pressure?

    <p>1.29 atm</p> Signup and view all the answers

    If 0.00810 mol of neon gas occupies 214 mL, what volume would 0.00684 mol of neon gas occupy under the same conditions?

    <p>180.0 mL</p> Signup and view all the answers

    What is the expected volume of a gas at 227.0 °C and 600.0 torr if it initially occupies 800.0 mL at −23.0 °C and 300.0 torr?

    <p>1200 mL</p> Signup and view all the answers

    If a gas's volume is affected by both temperature and pressure changes, what would happen to the volume if the pressure increases while temperature remains constant?

    <p>The volume decreases</p> Signup and view all the answers

    What principle explains the behavior of gases under different temperature and pressure conditions in a closed system?

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

    What would be the moles of gas added if the volume increased from 300 mL to 600 mL while maintaining constant temperature and pressure?

    <p>0.02 mol</p> Signup and view all the answers

    What is the new volume of a balloon that initially holds 1.90 L of helium gas and has 0.0210 mol of additional helium added?

    <p>2.14 L</p> Signup and view all the answers

    If a gas occupies an 8.00 mL flexible-walled container and its pressure is doubled, the absolute temperature is quadrupled, and 15% of the gas leaks out, what is the new volume?

    <p>9.56 mL</p> Signup and view all the answers

    When a gas is heated at constant pressure, what happens to its volume?

    <p>It increases.</p> Signup and view all the answers

    What is the initial pressure of air inside a bubble if its volume increases by a factor of 10 when the temperature changes from 4.55°C to 18.45°C?

    <p>0.740 atm</p> Signup and view all the answers

    In an experiment, how many grams of helium were added to a cylinder if the volume was changed from 2.00 L to 2.70 L?

    <p>0.90 g</p> Signup and view all the answers

    If a balloon of air occupies a volume of 10.0 L at 25.0 °C and 1.00 atm, what temperature was it initially at if it occupied 9.40 L and had a pressure of 0.939 atm?

    <p>30.0 °C</p> Signup and view all the answers

    What happens to the volume of a gas when more gas is added to a container while keeping temperature and pressure constant?

    <p>The volume increases.</p> Signup and view all the answers

    If a flexible container starts with a volume of 5.120 L and contains 8.500 mol of gas, what is the final number of moles if the final volume is 18.10 L?

    <p>12.950 mol</p> Signup and view all the answers

    Study Notes

    Gases - Learning Guide 5.1 & 5.2

    • Desired Learning Competencies:
      • Interpret gas laws in relation to pressure, volume, temperature, and amount of gas.
      • Solve mathematical problems using gas laws.
      • Explain practical applications of gas laws.

    Gas Laws (Boyle's, Charles', Avogadro's, Combined Gas Law)

    • Learning Guide, 521
    • Variables to consider: T (temperature), P (pressure), V (volume), and n (amount of gas)

    Different Conditions Affecting Balloon Size

    • Balloon left in the sun: It will expand
    • Balloon brought to higher elevation: It will expand
    • Pumping more gas into a balloon: It will expand

    Temperature (T)

    • Temperature measures the speed of gas particles.
    • Kelvin scale does not have negative values.
    • Zero Kelvin (0 K) is absolute zero.
    • Conversion: TKelvin = TCelsius + 273.15

    Pressure (P)

    • Pressure is the frequency of gas particle collisions with container walls.
    • At sea level, atmospheric pressure is 1 atm.
    • Unit conversions:
      • 1 atm = 101,325 Pa
      • 1 atm = 760 torr
      • 1 atm = 760 mmHg
      • 1 atm = 100,000 Pa

    Standard Temperature and Pressure (STP)

    • Temperature: 273.15 K or 0°C
    • Pressure: 1 atm

    Normal Temperature and Pressure (NTP)

    • Temperature: 293.15 K or 20°C
    • Pressure: 1 atm

    Amount of Gas (n)

    • Expressed in moles.
    • At STP, one mole of gas occupies 22.4 L at 1 atm pressure.

    Boyle's Law

    • Pressure and volume are inversely proportional at constant temperature.
    • P1V1 = P2V2

    Sample Problems

    • Various problem examples relating to Boyle's Law, including solutions

    Applications of Boyle's Law

    • Breathing
    • Inflating tires
    • Soda bottles
    • Syringes
    • Scuba diving

    Charles' Law

    • Volume and absolute temperature are directly proportional at constant pressure.
    • V1/T1 = V2/T2
    • Practice problems illustrating Charles' Law principles included.

    Applications of Charles' Law

    • Hot air balloons
    • Ping Pong balls

    Avogadro's Law

    • Volume and number of moles are directly proportional at constant temperature and pressure.
    • V1/n1 = V2/n2
    • Practical examples illustrated, including solutions

    Sample Problems

    • Problems related to applying Avogadro's Law, with solutions clearly shown

    Learning Check

    • Various problems applying the gas laws.
    • Detail solutions for each exercise.

    Combined Gas Law

    • Relates volume, pressure, and temperature of a constant quantity of gas (at constant moles of gas).
    • P1V1/T1 = P2V2/T2

    Cooling and heating at constant volume

    Sample problems

    • Problems involving combined gas law principles, calculations shown

    Learning Check

    • Additional problems related to concepts

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    Description

    This quiz covers the critical aspects of gas laws including Boyle's, Charles', Avogadro's, and the Combined Gas Law. It aims to reinforce understanding of pressure, volume, temperature, and their interrelationships through practical applications and problem-solving. Prepare to interpret various conditions affecting gas behavior, particularly in relation to balloons.

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