Gas Laws and Charles's Law Quiz
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Questions and Answers

What effect does a one-degree increase in temperature have on the volume of a gas at 0℃ according to Charles's law?

  • The volume decreases by $V_o/273$
  • The volume increases by $V_o/273$ (correct)
  • The volume remains constant
  • The volume doubles

    • Which equation correctly represents the relationship between volume and absolute temperature according to Charles's law?

  • $V_1 = P imes T_1$
  • $V_1 = P / T_1$
  • $V_1 = k imes T_1$ (correct)
  • $V_1 = T_1 / k$

    • What happens to the volume of a gas at -273°C according to Charles's law?

  • It reaches its maximum volume
  • It equals the volume at 0°C
  • It becomes negative
  • It becomes zero (correct)

    • Which statement best defines Charles's law?

    <p>Volume is directly proportional to absolute temperature at constant pressure</p> Signup and view all the answers

    What is the formula used to express the relationship between the volumes and temperatures of two gas states according to Charles's law?

    <p>$ rac{V_1}{V_2} = rac{T_1}{T_2}$</p> Signup and view all the answers

    Which condition is necessary for Charles's law to hold true?

    <p>Constant pressure</p> Signup and view all the answers

    What occurs when the temperature of a gas reaches absolute zero, according to the concept of absolute temperature?

    <p>All gas molecules cease movement</p> Signup and view all the answers

    What does the combined gas equation specifically account for?

    <p>The simultaneous effects of temperature and pressure on volume</p> Signup and view all the answers

    What is the molar mass of acetylene (C2H2)?

    <p>26 g/mol</p> Signup and view all the answers

    Using the ideal gas law, what is the volume of 5.0 g of acetylene at 50°C and 740 mm Hg?

    <p>8.51 L</p> Signup and view all the answers

    Calculate the pressure of a gas that occupies 1 L at 27°C using the ideal gas equation.

    <p>24.63 atm</p> Signup and view all the answers

    What is the mass of oxygen gas occupying 320 ml at 17°C and 2 atm?

    <p>0.860 g</p> Signup and view all the answers

    According to Charles's law, what is the final temperature when the gas volume increases from 350 ml to 400 ml at a constant pressure?

    <p>357.71 K</p> Signup and view all the answers

    What is the relationship described by Boyle's law?

    <p>Volume is inversely proportional to pressure at constant temperature.</p> Signup and view all the answers

    According to Charles's law, how does volume relate to absolute temperature?

    <p>Volume is directly proportional to absolute temperature at constant pressure.</p> Signup and view all the answers

    What does the combined gas equation represent?

    <p>The relationship between pressure, volume, and temperature of a gas.</p> Signup and view all the answers

    Which of the following gases behaves most like an ideal gas?

    <p>Helium (He)</p> Signup and view all the answers

    What is the value of the universal gas constant R based on the given conditions at NTP?

    <p>0.0821 atm.L/mol.K</p> Signup and view all the answers

    What happens to the volume of a gas if the absolute temperature is halved while pressure remains constant?

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

    Which equation represents the relationship between pressure, volume, and temperature for a given mass of gas?

    <p>$PV = nRT$</p> Signup and view all the answers

    What characterizes a real gas in comparison to an ideal gas?

    <p>Real gases deviate from ideal behavior at low temperature and high pressure.</p> Signup and view all the answers

    What will be the final pressure of the hydrogen gas when mixed in a 5 litre vessel?

    <p>225 mm of Hg</p> Signup and view all the answers

    How much CO2 gas will the fire extinguisher deliver at NTP given it contains 4.4 kg?

    <p>2238.33 litres</p> Signup and view all the answers

    What is the molecular weight of CO2 used in the calculations?

    <p>44</p> Signup and view all the answers

    Given the mass of a gas and its initial conditions, which equation is correctly used to find the molecular mass?

    <p>PV=M/RT</p> Signup and view all the answers

    What is the final pressure of the oxygen gas when mixed in a 5 litre vessel?

    <p>40 mm of Hg</p> Signup and view all the answers

    What is the total pressure of the gaseous mixture of hydrogen and oxygen?

    <p>265 mm of Hg</p> Signup and view all the answers

    Which value corresponds to the universal gas constant R in atm litre K-1 mol-1 used in the gas law equations?

    <p>0.0821</p> Signup and view all the answers

    To convert 730 mm Hg to atm for calculations, which of the following approximates the conversion correctly?

    <p>0.96 atm</p> Signup and view all the answers

    What is the final calculated volume of the gas based on the provided formula?

    <p>1.127 litre</p> Signup and view all the answers

    How can the molecular mass of the gas in the evacuated flask be determined?

    <p>Using the ideal gas equation rearranged to find M</p> Signup and view all the answers

    What is the molecular mass of gas A based on the given parameters?

    <p>48.93 g.m.</p> Signup and view all the answers

    If 3g of gas B is added to the flask and the pressure changes, what is the ratio of molecular masses of gases A and B?

    <p>1:3</p> Signup and view all the answers

    What is the pressure expected from 2 moles of ammonia in a 5-litre flask at 27°C using the ideal gas law?

    <p>9.852 atm</p> Signup and view all the answers

    What happens to the pressure exerted by a volatile liquid when the temperature of the system increases?

    <p>Pressure increases due to increased vaporization</p> Signup and view all the answers

    What is the molecular mass of the gas if the weight of gas in the evacuated flask is 0.977 g?

    <p>80.20 g.m.</p> Signup and view all the answers

    What would be the pressure of 0.50 g.m. of a volatile liquid in a 500 ml globe at 118°C when vaporized?

    <p>190 mm Hg</p> Signup and view all the answers

    What is the molecular mass of the given liquid calculated using the formula M = ( \frac{ WRT }{ PV } )?

    <p>59.76 g.m</p> Signup and view all the answers

    When the balloon is taken from 5°C to 25°C, what is the final volume of the gas inside based on Charles's Law?

    <p>1.045 ltr</p> Signup and view all the answers

    How many moles of an ideal gas are present in 50 ml exerting a pressure of 770 mm Hg at 25°C?

    <p>2.07 x 10^-3</p> Signup and view all the answers

    According to Dalton's law of partial pressure, how is the total pressure of a gas mixture determined?

    <p>It is the sum of the partial pressures of the component gases.</p> Signup and view all the answers

    What do n₁, n₂, and n₃ represent in the context of Dalton's law of partial pressure?

    <p>The number of moles of each component gas</p> Signup and view all the answers

    In the calculation for the number of moles, which of the following values is incorrectly substituted when using the ideal gas law?

    <p>Temperature as 273 K</p> Signup and view all the answers

    If pressure increases while temperature and volume remain constant, what happens to the number of moles in accordance with the ideal gas law?

    <p>The number of moles decreases.</p> Signup and view all the answers

    What happens to the balloon's gas volume according to Charles's Law if ambient temperature exceeds the initial temperature?

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

    Study Notes

    States of Matter

    • Matter exists in three physical states: gaseous, liquid, and solid.
    • Water exists in three physical states: ice, liquid water, and steam.

    Gaseous State

    • A gaseous state of matter has neither a fixed shape nor a fixed volume.

    Gas Laws

    • Boyle's Law: At constant temperature, the volume of a given mass of gas is inversely proportional to its pressure.
    • Charles's Law: At constant pressure, the volume of a given mass of gas is directly proportional to its absolute temperature.
    • Combined Gas Law: Combines Boyle's and Charles's laws, relating pressure, volume, and temperature of a gas.
    • 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 individual gases.
    • Graham's Law of Diffusion: The rate of diffusion of a gas is inversely proportional to the square root of its molar mass.

    Ideal Gas Equation

    • The ideal gas equation is PV = nRT, where:
      • P is pressure
      • V is volume
      • n is the number of moles
      • R is the ideal gas constant
      • T is temperature

    Ideal Gas

    • An ideal gas is a gas that perfectly obeys the gas laws

    Absolute Zero

    • Theoretical temperature at which the volume of a gas becomes zero at constant pressure. -273°C or 0 Kelvin (0 K)

    Concepts

    • Real gas: A real gas does not obey the ideal gas laws at all temperatures and pressures, unlike an ideal gas.
    • Conditions for Ideal Behavior: Gases behave ideally at low pressures and high temperatures.

    Mole Concept Examples

    • Calculations involving quantities like pressure, volume, moles, and temperature for a variety of gases

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    Description

    Test your understanding of gas laws, particularly Charles's law, and the ideal gas law. This quiz covers various concepts, including the relationship between volume and temperature, absolute zero, and the molar mass of gases. Perfect for students studying chemistry and gas behavior.

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