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Questions and Answers
Which of the following elements exists as a gas at 25°C and 1 atmosphere?
Which of the following elements exists as a gas at 25°C and 1 atmosphere?
Gases have a tendency to mix evenly when confined to the same container.
Gases have a tendency to mix evenly when confined to the same container.
True
What is the boiling point of hydrogen cyanide (HCN) at standard conditions?
What is the boiling point of hydrogen cyanide (HCN) at standard conditions?
26°C
The standard unit of pressure measurement is ______.
The standard unit of pressure measurement is ______.
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Match the following gases with their boiling points:
Match the following gases with their boiling points:
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What is the pressure in atmospheres in the cabin if the barometer reading is 688 mmHg?
What is the pressure in atmospheres in the cabin if the barometer reading is 688 mmHg?
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Boyle's Law states that the volume of a gas is directly proportional to its pressure at constant temperature.
Boyle's Law states that the volume of a gas is directly proportional to its pressure at constant temperature.
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What is the formula for the Ideal Gas Equation?
What is the formula for the Ideal Gas Equation?
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The temperature must be in __________ when using Charles' law.
The temperature must be in __________ when using Charles' law.
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Match the gas laws with their corresponding relationships:
Match the gas laws with their corresponding relationships:
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Study Notes
Elemental Gases
- Elements that exist as gases at 25°C and 1 atmosphere are considered elemental gases.
Common Gases
- Several elements exist as gases at 1 atm and 25°C, including:
- H2 (molecular hydrogen)
- N2 (molecular nitrogen)
- O2 (molecular oxygen)
- O3 (ozone)
- F2 (molecular fluorine)
- Cl2 (molecular chlorine)
- He (helium)
- Ne (neon)
- Ar (argon)
- Kr (krypton)
- Xe (xenon)
- Rn (radon)
- Several compounds are also gases at 1 atm and 25°C, including:
- HF (hydrogen fluoride)
- HCL (hydrogen chloride)
- HBr (hydrogen bromide)
- HI (hydrogen iodide)
- CO (carbon monoxide)
- CO2 (carbon dioxide)
- CH4 (methane)
- C2H2 (acetylene)
- NH3 (ammonia)
- NO (nitric acid)
- NO2 (nitrogen dioxide)
- N2O (nitrous oxide)
- SO2 (sulfur dioxide)
- SF6 (sulfur hexafluoride)
- H2S (hydrogen sulfide)
- HCN (hydrogen cyanide)
Physical Characteristics of Gases
- Gases assume the volume and shape of their containers.
- Gases are the most compressible state of matter.
- Gases mix evenly and completely when confined to the same container.
- Gases have much lower densities than liquids and solids.
Factors Affecting Gases
- Key factors influencing gas behavior include:
- Pressure (atm)
- Volume (L)
- Temperature (°K)
- Number of moles (n)
Pressure
- Pressure is defined as force per unit area.
- Units of Pressure:
- 1 pascal (Pa) = 1 N/m^2
- 1 atm = 760 mmHg = 760 torr
- 1 atm = 101,325 Pa
Manometers
- Manometers are used to measure gas pressures.
- Two types of manometers exist: closed-tube and open-tube.
Boyle’s Law
- States that at constant temperature, the volume of a gas is inversely proportional to its pressure.
- The mathematical expression is: P1V1 = P2V2
Charles’s and Gay-Lussac’s Law
- States that at constant pressure, the volume of a gas is directly proportional to its absolute temperature.
- Mathematical expression is: V1/T1 = V2/T2
Avogadro’s Law
- States that at constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of gas.
- Mathematical expression is: V1/n1 = V2/n2
Ideal Gas Equation
- Combines Boyle's, Charles's, and Avogadro's laws into a single equation:
- PV = nRT
- Where:
- P is pressure (atm)
- V is volume (L)
- n is the number of moles
- R is the ideal gas constant (0.0821 L ‧ atm/mol ‧ K)
- T is the absolute temperature (K)
Standard Temperature and Pressure (STP)
- Standard temperature and pressure are defined as 0°C (273.15 K) and 1 atm.
- At STP, 1 mole of an ideal gas occupies 22.414 L.
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Description
Test your knowledge on elemental gases that exist at 25°C and 1 atmosphere. This quiz covers common gases, their molecular structures, and some important gaseous compounds. Challenge yourself to identify and understand the characteristics of various gases.
