Does A Substance Exist As A Gas, Liquid, Or Solid?

whether A Substance Exists As A Gas Liquid Or Solid Depen

Whether a substance exists as a gas, liquid, or solid depends on the balance between the kinetic energy of its particles and the strength of the interactions between the particles.

Match the property with s, l or g:

• Expands to fill the container — B. gas
• A fixed volume that takes the shape of the container it occupies — C. liquid
• A definite shape and volume — A. solid
• Arrangement of particles: randomly arranged, disorganized and far apart — B. gas
• Fixed arrangement of very close particles — A. solid
• Density is low (< 0.01 g/mL) — B. gas
• Particles are moving very fast — B. gas
• Interactions between the particles are very strong — A. solid
• densities are around 1 g/mL — C. liquid
• No interactions between the particles — B. gas

Match up the gas name with the definition:

1. Boyle’s Law: — A. For a fixed amount of gas at constant temperature, the pressure and volume of the gas are inversely related.
2. Charles’s Law: — G. For a fixed amount of gas at constant pressure, the volume of the gas is proportional to its Kelvin temperature.
3. Gay–Lussac’s (Amonton's) Law: — H. For a fixed amount of gas at constant volume, the pressure of a gas is proportional to its temperature in Kelvin.
4. The combined gas law: — E. All three gas laws (Boyle’s, Charles’, and Gay-Lussac) can be combined into one equation.
5. Avogadro’s Law: — C. When the pressure and temperature are held constant, the volume of a gas is proportional to the number of moles present.
6. Standard molar volume: — F. At STP, 1 mole of any gas has a volume of 22.4 L.
7. The ideal gas law: — D. All four properties of gases (P, V, n, T) can be combined into a single equation which can operate outside of STP.
8. Dalton’s law: — B. The total pressure (P_total) of a gas mixture is the sum of the partial pressures of its component gases.

Pressure is calculated from (Force / ____) — Area

The units of pressure are — All of the above (mm Hg, torr, pounds per square inch (psi), Pascals (Pa), atmospheres (atm))

The tires on a road bike are inflated to 90. psi. Convert this pressure to mm Hg:

• 1 atm = 14.7 psi = 760 mm Hg

Calculation: 90 psi * (760 mm Hg / 14.7 psi) ≈ 4,653.1 mm Hg

If a 4.0-L container of helium gas has a pressure of 10.0 atm, what pressure does the gas exert if the volume is increased to 6.0 L? — 6.67 atm (using Boyle's Law: P1V1 = P2V2)

Calculate the Kelvin temperature to which 10.0 L of a gas at 27°C would have to be heated to change the volume to 12.0 L. — Approximately 300 K (using Charles's Law: V1/T1 = V2/T2)

When performing gas law calculations, the units of temperature should always be — Kelvin

If a plastic container of food at 1.0°C and 750 mm Hg is heated in a microwave to 80.°C, what is the new pressure inside the container? — 795 mm Hg (using Gay-Lussac's Law)

At STP, 1 mole N₂ gas occupies approximately 22.4 L, and this accounts for 6.022 x 10²³ molecules and 28.0 g of nitrogen.

How many moles are contained in 2.0 L of N₂ at standard temperature and pressure? — 0.089 mol

How many moles are contained in 5.33 L of O₂ at standard temperature and pressure? — 0.238 mol

How many moles of gas are contained in a typical human breath that takes in 0.50 L of air at 1.0 atm pressure and 37°C? — Approximately 0.021 mol

A sample of exhaled air contains four gases with the following partial pressures: N₂ (563 mm Hg), O₂ (118 mm Hg), CO₂ (30 mm Hg), and H₂O (50 mm Hg). What is the total pressure of the sample? — 761 mm Hg

An air-filled balloon has a volume of 215 mL at 23°C. If the temperature drops to –65°C, will the balloon now expand, stay the same, or shrink? — Shrink (assuming constant pressure and n)

What observation do you make as this reaction goes forward? (2 Na(s) + 2 H₂O(l) → H₂(g) + 2 NaOH(aq)) — Bubbling from the liquid, disappearance of solid sodium, formation of solution, and possible color changes

Which cylinder at STP will contain the greatest number of gas particles? — All contain the same number since volume, temperature, and pressure are the same for equal volumes of gases per Avogadro's law.

For a deep dive, a scuba diver uses a mixture of helium and oxygen with a total pressure of 7.28 atm. If the oxygen has a partial pressure of 1,600 mm Hg, what is the partial pressure of the helium in mm Hg? — 2,183 mm Hg (Total pressure = partial pressures sum)

Consider the reaction: Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g). What volume of H₂ gas at STP can be generated when 134 g of zinc reacts? — Approximately 45.9 L (using stoichiometry and molar volume)

Dry air is 78.09% nitrogen, 20.95% oxygen, 0.93% argon, 0.039% CO₂. Which greenhouse gas has shown a marked increase in atmospheric concentrations in the last 100 years? — Carbon dioxide (CO₂)

Elevated global temperatures result in the air above land being Term 1 and having Term 2, while the air above the ocean becomes Term 3 and with Term 4. (This appears incomplete, but generally, during warming, air over land becomes drier and experiences more extreme conditions.)

Paper For Above instruction

Understanding the physical states of matter — solids, liquids, and gases — is fundamental to grasping the principles of chemistry. The states are primarily determined by the interplay between the kinetic energy of particles and the forces of attraction among them. Solids are characterized by a fixed shape and close-packed particles held together by strong intermolecular forces. These particles vibrate around fixed points, resulting in definite shape and volume. Liquids possess a definite volume but take the shape of their container, with particles more loosely packed than solids and capable of flowing past each other. Gases, however, expand to fill their containers because their particles move rapidly and are spaced far apart, with negligible intermolecular forces.

Key properties distinguish these states. Solids have high densities and fixed shapes, with particles arranged in ordered structures. Liquids have intermediate densities and indefinite shapes, with particles arranged randomly but close enough to maintain volume. Gases have low densities, expand to fill containers, and have particles that move rapidly with weak interactions among them. These properties are critical in understanding phase behavior and equilibriums in chemical systems.

The behavior of gases is described by several fundamental laws, such as Boyle’s law, Charles's law, Gay–Lussac’s law, and Avogadro's law. Boyle’s law states that, at constant temperature, pressure and volume are inversely proportional (P₁V₁=P₂V₂). Charles’s law asserts that, at constant pressure, volume and Kelvin temperature are directly proportional (V₁/T₁=V₂/T₂). Gay–Lussac’s law indicates that for constant volume and moles, pressure and temperature are proportional (P₁/T₁=P₂/T₂). The ideal gas law combines these and other properties into PV=nRT, where n is the number of moles and R is the ideal gas constant, allowing comprehensive description of gases under various conditions.

Pressure measurement is fundamental in many scientific and practical applications. It is calculated as force divided by area and measured in units such as mm Hg, atmospheres (atm), Pascals (Pa), pounds per square inch (psi), and torr. Conversion among these units is often necessary in applications like tire pressure or laboratory experiments. For example, to convert 90 psi to mm Hg, the pressure is first converted to atmospheres using the relation 1 atm = 14.7 psi and then multiplied by 760 mm Hg per atm, resulting in approximately 4,653.1 mm Hg.

The principles of gas laws are applied in calculations involving changes in pressure, volume, and temperature, often requiring the use of Kelvin temperature for accuracy. For instance, increasing the temperature of a gas at constant volume results in a proportional increase in pressure, as per Gay-Lussac’s law. Conversion between Celsius and Kelvin is straightforward: add 273.15 to Celsius temperatures. The relationships among these variables aid in understanding phenomena such as the behavior of air in weather balloons or the release of gases during chemical reactions.

Quantitative problems involving gases often utilize molar volume at STP (22.4 L per mole for gases at standard conditions), enabling the calculation of moles and the number of particles based on volume. For instance, 2.0 L of N₂ contains approximately 0.089 mol, while 5.33 L corresponds to about 0.238 mol. These calculations are grounded in the ideal gas law and Avogadro’s principle.

Understanding partial pressures is crucial in analyzing gas mixtures such as air. For example, the partial pressure of oxygen in exhaled air can be determined by multiplying the total pressure by the fractional partial pressure of oxygen, which helps in medical and environmental assessments. The total pressure of exhaled air is the sum of its partial pressures, approximately 761 mm Hg in a typical sample.

The behavior of gases under changing conditions, such as temperature shifts, influences phenomena like the expansion or shrinking of balloons. At lower temperatures, gases contract, leading to volume reduction if the pressure remains constant. Additionally, reactions producing gases, such as sodium reacting with water, produce observable effects like bubbling due to hydrogen production, illustrating gas evolution in chemical processes.

For specific applications such as diving, understanding partial pressures within mixtures like helium and oxygen is vital for avoiding issues like nitrogen narcosis or oxygen toxicity. Calculations involve summing partial pressures and applying Dalton’s law to determine individual gas contributions.

Chemical equations further illustrate gas behavior. The reaction Zn + 2 HCl → ZnCl₂ + H₂ demonstrates stoichiometry's application to gas volumes at STP, where 134 g of zinc produces approximately 45.9 liters of hydrogen gas.

Environmental concerns such as climate change are closely associated with greenhouse gases, especially carbon dioxide, which has significantly increased in atmospheric concentration over the past century. These gases trap infrared radiation, leading to global warming. Elevated temperatures cause land to heat and dry out, while ocean temperatures also rise, causing phenomena like sea level rise, melting ice caps, and enhanced weather extremes.

In conclusion, the study of states of matter and gas laws provides essential insights into natural and industrial processes. Recognizing how physical properties and laws govern the behavior of matter under various conditions enables scientists and engineers to develop solutions for environmental challenges, improve technologies, and deepen our understanding of the physical universe.

References

• Atkins, P., & de Paula, J. (2014). Physical Chemistry (10th ed.). Oxford University Press.
• Chang, R., & Goldsby, K. (2016). Chemistry (12th ed.). McGraw-Hill Education.
• McQuarrie, D. A., & Simon, J. D. (1997). Physical Chemistry: A Molecular Approach. University Science Books.
• Laidler, K., Meiser, J. H., & Sanctuary, B. C. (1999). Physical Chemistry (3rd ed.). Houghton Mifflin.
• LibreTexts. (2020). Gas Laws. https://chem.libretexts.org
• Brown, T. L., LeMay, H. E., Bursten, B. E., Murphy, C., & Woodward, J. (2018). Chemistry: The Central Science (14th ed.). Pearson.
• Oxtoby, D. W., Gillis, H. P., & Butler, S. (2019). Principles of Modern Chemistry (8th ed.). Cengage Learning.
• Excel Chemistry. (2019). Practical Gas Law Calculations. https://www.excelchemistry.com
• EPA. (2021). Greenhouse Gases and Climate Change. U.S. Environmental Protection Agency.
• IPCC. (2021). Climate Change 2021: The Physical Science Basis. Intergovernmental Panel on Climate Change.