Index of Chemical Terms and Concepts

Index of Terms and Concepts (Draft 5.16.01)

Click-on the name of the term or concept for a complete description, discussion, graphics, animations, and links to additional terms.

Avogadro''s Hypothesis

Avogadro's Hypothesis states that for different gases at the same volume, temperature, and pressure, there are equal moles and equal number of gas molecules present.

Avogadro''s Law

The volume of a gas is proportional to n, the number of moles of the gas.

V₁n₂ = V₂n₁(T,P constant)

Boyle's Law

The volume of a gas is inversely proportional to its pressure.

P₁V₁ = P₂V₂(T, n constant)

Charles's Law and Gay-Lussac's Law

The volume of a gas is proportional to its absolute temperature.

V₁T₂ = V₂T₁ ( P, n constant)

When measured at the same pressure and temperature, the volume of a gas reactants and products are in ratios of simple whole numbers.

Collecting a Gas Over Water

An experimental procedure for collecting a gas in a tube by the displacement of water. Dalton's law of partial presures is applied to calculate the pressure of the gas collected. The vapor pressure of water is subtracted from the total pressure in order to obtain the partial pressure of the gas collected.

Combined Gas Laws

The combined gas law relates the volume, pressure, and temperature of a gas from its initial condition to its final condition.

Diffusion

Diffusion refers to the movement of gas molecules (Gas A) from a space where the Gas A molecule are concentrated to a space or through space in which another type of gas molecules (Gas B) are present. Gas A molecules moves from a more concentration space to a less concentrated space, until the concentration of Gas A is homogeneous. diffusionV8.html

Dalton's Law of Partial Pressures

Dalton's law of partial pressures states that the total pressure exerted by a mixture of gases is the sum of partial pressure of each individual gas present.

P_total = P₁ + P₂ + P₃ + . .

Effusion

Effusion refers to the movement of gas molecules from an enclosed space into an evacuated space through a small opening. Effusion2.html

Gas Constant, R

0.08206 L atm/mol K

Graham's Law of Effusion

Graham's Law of Effusion states that the rate of effusion of a gas is inversely proportional to the square root of its density.

Ideal Gas Law and Ideal Gas

The ideal gas law is a mathematical model for accounting for the physical parameters (P, V, T, n) of ideal gases. PV = nRT

An ideal gas is a hypothetical gas whose pressure-volume-temperature physical parameters can be completely accounted for by the ideal gas equation.

Kinetic Energy

Kinetic energy is energy due to motion. KE = (1/2)mv²

Kinetic Molecular Theory of Gases

The kinetic molecular theory is a molecular level representation and a mathematical way of describing and accounting for the physical behavior of gases. The kinetic molecular theory is a model. There are five assumption of this theory.

Maxwell Speed Distribution Curve

Molecular Weight of Gas

Partial Pressure

The partial pressure of a gas, in a mixture of gases, is equal to its mole fraaction times the total pressure. P₁ = X₁P_T

The partial pressure of a gas, in a mixture of gases, can be calulated using the ideal gas equation.

Pressure

Root-Mean-Square Speed (rms)

The root-mean-square speed, u, is the square root of the average speeds of the molecules in a sample of gas at a specific temperature and pressure.

Standard Temperature and Pressure (STP)

Stoichiometry

Temperature

van der Waals gas

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Car batter PbbatteryV8web.html

Index of Terms and Concepts (Draft 5.16.01) Click-on the name of the term or concept for a complete description, discussion, graphics, animations, and links to additional terms.
Avogadro''s Hypothesis	Avogadro's Hypothesis states that for different gases at the same volume, temperature, and pressure, there are equal moles and equal number of gas molecules present.
Avogadro''s Law	The volume of a gas is proportional to n, the number of moles of the gas. V₁n₂ = V₂n₁(T,P constant)
Boyle's Law	The volume of a gas is inversely proportional to its pressure. P₁V₁ = P₂V₂(T, n constant)
Charles's Law and Gay-Lussac's Law	The volume of a gas is proportional to its absolute temperature. V₁T₂ = V₂T₁ ( P, n constant) When measured at the same pressure and temperature, the volume of a gas reactants and products are in ratios of simple whole numbers.
Collecting a Gas Over Water	An experimental procedure for collecting a gas in a tube by the displacement of water. Dalton's law of partial presures is applied to calculate the pressure of the gas collected. The vapor pressure of water is subtracted from the total pressure in order to obtain the partial pressure of the gas collected.
Combined Gas Laws	The combined gas law relates the volume, pressure, and temperature of a gas from its initial condition to its final condition.

Diffusion	Diffusion refers to the movement of gas molecules (Gas A) from a space where the Gas A molecule are concentrated to a space or through space in which another type of gas molecules (Gas B) are present. Gas A molecules moves from a more concentration space to a less concentrated space, until the concentration of Gas A is homogeneous. diffusionV8.html
Dalton's Law of Partial Pressures	Dalton's law of partial pressures states that the total pressure exerted by a mixture of gases is the sum of partial pressure of each individual gas present. P_total = P₁ + P₂ + P₃ + . .
Effusion	Effusion refers to the movement of gas molecules from an enclosed space into an evacuated space through a small opening. Effusion2.html
Gas Constant, R	0.08206 L atm/mol K
Graham's Law of Effusion	Graham's Law of Effusion states that the rate of effusion of a gas is inversely proportional to the square root of its density.

Ideal Gas Law and Ideal Gas	The ideal gas law is a mathematical model for accounting for the physical parameters (P, V, T, n) of ideal gases. PV = nRT An ideal gas is a hypothetical gas whose pressure-volume-temperature physical parameters can be completely accounted for by the ideal gas equation.
Kinetic Energy	Kinetic energy is energy due to motion. KE = (1/2)mv²
Kinetic Molecular Theory of Gases	The kinetic molecular theory is a molecular level representation and a mathematical way of describing and accounting for the physical behavior of gases. The kinetic molecular theory is a model. There are five assumption of this theory.

Maxwell Speed Distribution Curve
Molecular Weight of Gas
Partial Pressure	The partial pressure of a gas, in a mixture of gases, is equal to its mole fraaction times the total pressure. P₁ = X₁P_T The partial pressure of a gas, in a mixture of gases, can be calulated using the ideal gas equation.
Pressure
Root-Mean-Square Speed (rms)	The root-mean-square speed, u, is the square root of the average speeds of the molecules in a sample of gas at a specific temperature and pressure.

Standard Temperature and Pressure (STP)
Stoichiometry
Temperature
van der Waals gas