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Questions and Answers
Which of the following gases will effuse most slowly under the same conditions?
Based on the definition of diffusion and effusion, which examples are correctly matched?
Identify the factor that determines rates of diffusion and effusion for different molecules at a given temperature.
Which of the following is an assumption of the kinetic molecular theory of gases?
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The movement of gas is greatly affected by ___.
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At what pressure (atm) is the nitrogen gas sample collected when 48.40 g of NaN3 decomposes?
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If 10.30 L of ammonia gas at 20.0 degree Celsius and 0.989 atm is created, how many liters of water at STP are required?
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How many grams of CaC2 would be needed to produce 10.00 L of acetylene at STP?
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How many moles are in a 22.40 L sample of an ideal gas at STP?
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When solving gas stoichiometry problems, which of the following is correctly matched?
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What is known as the quantitative study of reactants and products in a chemical reaction?
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How many grams of oxygen are in a 5.0 L cylinder containing oxygen gas at 20.00 degree Celsius and 735 mmHg?
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What will be the pressure inside a container with 0.40 moles of oxygen gas at 350 K and a volume of 4.0 L?
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A gas mixture contains 2.5 mol N2 and 9.7 mol CO2, and has a pressure of 2.30 atm. What is the partial pressure of each gas?
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If four gases exert a total pressure of 6 mmHg, with gas A and B exerting 2 mmHg each, and gas C exerting 0.20 mmHg, how much pressure does gas D exert?
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What refers to the pressure each gas exerts in a mixture?
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In an ideal gas, if everything is held constant, doubling the volume will ___ the pressure.
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What is the new temperature of helium gas when its volume is 90.0 mL and pressure is 3.20 atm?
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What is the final pressure of a hydrogen balloon after it is inflated from 2L to 6L with an initial pressure of 1.50 atm?
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With pressure constant, if the temperature of a gas is increased from 30 degree Celsius to 90 degree Celsius, the volume will ___?
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If you collect 22.4 L of oxygen gas at standard conditions, you will have ___.
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Study Notes
Gas Properties and Behavior
- Gases diffuse and effuse, with diffusion being the spread of gas molecules and effusion referring to gas escaping through a small hole.
- Effusion rate is inversely related to the molar mass of the gas according to Graham's law.
Diffusion and Effusion Examples
- Examples of diffusion include a flat tire releasing air and incense sticks evaporating into the air.
- Examples of effusion include aerosol sprays discharging gas and a deflating balloon.
Factors Affecting Gas Behavior
- The rate of diffusion and effusion is primarily determined by the size of molecules and their molar mass.
- Kinetic molecular theory assumes gas particles have elastic collisions and that their temperature is related to average kinetic energy.
Reaction and Gas Calculations
- Understanding gas reactions involves using the ideal gas law (PV=nRT) and stoichiometry to relate moles, volume, and pressure at standard temperature and pressure (STP).
- STP conditions include 0°C (273.15 K) and 1 atm pressure, where 1 mole of an ideal gas occupies 22.4 L.
Pressure in Gas Mixtures
- Partial pressure refers to the pressure contributed by an individual gas in a mixture. The total pressure is the sum of all partial pressures.
- In a mixture where multiple gases are present, the total pressure can be calculated by adding individual partial pressures according to Dalton's law.
Gas Law Applications
- The ideal gas law helps determine changes in pressure, volume, and temperature of gases.
- Doubling the volume of an ideal gas at constant temperature will halve its pressure (Boyle's Law).
- Charles's Law states that at constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin.
Gas Molar Relationships
- At STP, collecting 22.4 L of a gas corresponds to 1 mole, equating to 6.02 x 10^23 molecules.
- Gas calculations often require conversions between volume and mass based on the ideal gas constant and molar relationships.
Practical Applications
- Tying concepts to real-world examples helps in understanding, such as how changes in balloon volume affect pressure or how gas mixtures behave under pressure.
- Practical applications of stoichiometry can assist in determining quantities required in chemical reactions involving gases, such as calculating grams of reactants needed for desired volumes of products.
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Description
This quiz covers key concepts in general chemistry, focusing on the principles of diffusion and effusion. Questions assess understanding of gas behavior and the factors influencing the rates of these processes. Test your knowledge and application of these fundamental concepts in chemistry.
