Chemistry Stack Exchange
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Questions tagged [gas-laws]

Physical and chemical laws describing the properties and behavior of gases. This tag currently applies to properties and laws concerning both ideal and real gases.

Physical and chemical laws describing the properties and behavior of gases; relationships between the pressure, volume, and temperatures of gases. Specific examples include, but are not limited to:

  • Ideal gas law: that gives us the ideal gas equation: pV = nRT
  • Henry's law: relates the mole fraction of a gas dissolved in solution to its partial pressure
  • Dalton's law: relates the partial pressure of gases to their mole fraction in the container
  • Raoult's law: relates the vapour pressure of immiscible solvents with their mole fractions
  • Charles' law: relates volume to temperature at constant pressure
  • Gay-Lussac's law: refers to two different laws: 1) The ratio between the volumes of the reactant gases and the gaseous products can be expressed in simple whole numbers. 2) The pressure of a gas of fixed mass and fixed volume is directly proportional to the gas's absolute temperature.
  • Avogadro's law: equal volumes of all gases, at the same temperature and pressure, have the same number of molecules
  • Amagat's law: According to Amagat’s law of partial volume, the total volume of a non-reacting mixture of gases at constant temperature and pressure should be equal to the sum of the individual partial volumes of the constituent gases
  • Graham's law: relates the rate of diffusion of a gas to its molar mass
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In Graham's law, is the rate of effusion only dependent on molar mass?

According to Graham's Law, the effusion rate of a gas is inversely proportional to the square root of the molar mass of the gas. However, consider this situation: We have s balloon with 1 mole of neon gas and another with 2 moles of neon gas. The…
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Do 1 mole of both dioxygen gas and its atoms occupy 22.4 litres at STP?

The ideal gas law states: One mole of an ideal gas will occupy a volume of $\pu{22.4 liters}$ at STP. Does this mean that both $\pu{1 mole}$ of $\ce{O}$ would occupy $\pu{22.4 L}$ (or if this doesn't usually occur in nature, say \pu{1 mole }of…
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Ideal Gas Equation Contradiction

You have a regular balloon, and you decide to heat it up. The gas particles inside the balloon will gain kinetic energy, and so, the gaseous particles will collide with the internal wall of the balloon with a higher frequency and more energy. This…
StopReadingThisUsername
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Will CO2 bubbles ever fully dissolve in water?

Background: Many aquarists keep freshwater planted tanks add $\ce{CO2}$ from a pressurized canister to their aquaria to promote plant growth. The injection is at a slow rate to get dissolved $\ce{CO2}$ in the neighborhood of 30 ppm. Methods vary,…
Phil Frost
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Best ways to compress and store tons of CO2?

We are looking at doing planet changing work, and removing CO2 from the atmosphere. The issue is storing the CO2. Please let us know the best ways to compress millions of tons of CO2, as we have limited storage space. For example, how much could we…
Jim Moore
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Why do Hydrogen and Helium have molar volumes higher than an ideal gas?

In my chemistry textbook, there is a table of the molar volumes for different gases. Most of them are below 22.42 l/mol, the ideal gas molar volume, but I noticed that hydrogen and helium do not. Hydrogen is 22.433 l/mol and helium is 22.434 l/mol.…
Noel
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Why are gas laws only applicable to gases?

Why are the gas laws (such as Boyle's Law, Charles's Law, and Avogadro's Law) only applicable to gas and not liquids or solids?
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Real Gas Equation

When a real gas has a pressure lower than the expected value from ideal gas (because of the intermolecular force of attraction) , we have - $$P_{\text{ideal}}= P_{\text{real}} + \frac{an^2}{V^2}$$ where a is the Van der Waal's constant for…
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Graph of compressibility factor vs pressure when real gas is assigned Z=1

Problem: According to the real gas equation, $Z = 1$ for an ideal gas and $Z$ is variable for a real gas. Suppose, in order to easy our calculations, we fixed $Z=1$ for a real gas and for ideal gas, $Z$ will become variable. $Z$ vs $P$ for an ideal…
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How to use gas laws to calculate the partial pressure of a gas that has partly condensed from a mixture?

A mixture of three gases N2, CO2 and O2 has a total pressure of 106000 Pa. The mixture is cooled to -100°C and the resulting pressure is found to have decreased to 82500 Pa. What gas is condensed and what is its partial pressure? (BP N2 = -196°C,…
somerandomperson222
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Using combined gas law to calculate the volume of dry hydrogen gas

Volume of wet hydrogen collected at room temperature: $\pu{40.48 mL}$, ambient pressure: $\pu{29.7 inHg}$ ($\pu{754 torr}$), ambient temperature: $\pu{295 K}$ ($\pu{22^\circ C}$), vapor pressure of water at $\pu{22^\circ C}$: $\pu{19.83 torr}$.…
most venerable sir
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Which gas is easier to compress, the ideal gas or a real gas?

Since the pressure of a real gas is less than that of the ideal gas and its volume is more than that of ideal gas, I am assuming that the real gas is difficult to compress in comparison to an ideal gas. Is my logic right? Also I'm looking for a…
Niharika
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Validity of Henry's Law for an Oxygen/Bitumen System?

Henry's Law is for a gas dissolved in a liquid and states P = kC where P is the partial pressure of the gas above the solution and C is the concentration of the gas dissolved in the liquid. The k is a "constant", that is, it is independent of P, C…
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Derivation of the van der Waals equation

I’m trying to rationalize the van der Waals equation for a non-ideal gas. I understand it conceptually, but I cannot finish the algebra: Begin with the ideal gas law: P V = n R T This is really: P(ideal) V(ideal) = n R T (1) Now consider the…
Michael Roberts
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What are the dimensions of a and b in van der Waal's real gas formula?

In the van der Waal's formula for real gases $\left( p+\frac{a}{V^2}\right)(V-b)=nRT$, what are the dimensions of $a$ and $b$? I learnt that $a$ is related to the average force of attraction between the molecules and $b$ is related to the total…
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