Chemistry Gas Law Flashcard

states the volume of a fixed amount of gas held at constant temperature varies inversely with pressure

Boyle’s Law

states the volume of a given amount of gas is directly proportional to its Kelvin temperature at constant pressure

Charles’ Law

states that equal volumes of gases at the same temp and pressure contain an equal number of particles

Avogadro’s Law

states the pressure of a fixed amount of gas varies directly with the kelvin temperature when the volume remains constant 

Gay-Lussac

Boyle’s equation

P₁V₁ = P₂V₂

Charles’ Equation

T₁/V₁​​= T₂ / V₂​​

Gay Lussac Equation

P₁ / T₁ = P₂ / T₂

Avogadro’s Equation

V₁ / n₁ = V₂ / n₂

Relationship between Boyle’s Law

Inverse (1 doubles other halves vice versa)

Charles’ Law Relationship

Direct Relation (As V increase T increases vice versa)

Gay Lussac Relationship

Direct relation (As Pressure increase temp increase vice versa)

Avogadro Relationship

Direct relation (As volume increase the particles increase vice versa)

states the relationship among pressure, temperature, and volume of a fixed amount of gas

Combined Gas Law

particles occupy a negligible volume and are far enough apart to exert minimal attractive or repulsive force on each other

Ideal Gas Law

Combined Gas Law equation

P₁V₁ / T₁ = P₂ V₂ / T₂

Ideal Gas Law Equation

Pv=nRT

In deal Gas law equation the constant R is what?

0.0821 L Atm / mol k

Molar Mass from Ideal Gas Equation

subsitute n= m/mm in Ideal and rearrange to MM = mRT/PV

Density from Derrived Ideal Gas

Subsitute M/V from M=mRT/PV —> D=PMM/RT

RMS Speed equation

M_rms = √3RT/MM

If given mass and they want molar mass what equation?

Molar Mass from Ideal Gas

If see density, pressure, temperature what equation?

Density derrived from Ideal

The constant R in Rms Speed equation is what?

8.314 J/Mol K

Rms Speed equation is what theory

Kinetic Molecular Theory

Diffusion and Effusion

Graham’s Law Rate₁ / Rate₂ = √MM₂/MM₁

Spreading through space

Diffusion

Effusion

Passing through tiny hole

Ideal Gases follow the assumption of….

Kinetic Molecular Theory

Characteristics of ideal gases

• No intermolecular attractive or repulsive force between particles or with their containers

• The particles are in constant random motion

• Collisions are perfectly elastic (no energy transferred)

• No gas is truly ideal, but most behave as ideal gases at a wide range of temperatures and pressure 

Ideal assumption

1. Very weak IMFS (DON’T COUNT)

2. Small Particle (DON'T COUNT)

Ideal assumption do apply if…

High temp and Low Pressure (IMF AND PARTICLES COUNT)

Real vs ideal Gas

Real gases deviate most from ideal gases at high P and low T

Polar molecules have larger attrative forces between particles

Polar gases do not behave as ideal gases

Large nonpolar gas particles occupy more space and deviate more from ideal gases

Stoichiometry of Reactions involve…..

Gas (REVIEW SOME EQUATIONS)

Stoichiometry and Volume

Coefficients in a balanced equation represent the volume ratio for gases

A balance equation helps find ratios for moles and gases volume not masses

All masses must be converted to moles or volume before used in ratio

Nature of Gases

Easily compressable

Has mass and fill container completely

Can move through each other quite rapidly (diffusion)

Exert Pressure (P depends on its temp)

Measuring Gases (units)

Moles (n)

Volume (v) (L or mL)

Temperature (T) (kelvin)

Pressure (P) (Atm, 760mm Hg, 760 Torr)

Volume

Gas expands uniformly to fill any container in which it is placed

Pressure is….

Force per unit area

Pressure units

1 atm= 100KPa

1 atm= 760 mm Hg = 101.3 kPA

Kinetic Molecular Theory

Explains the Gas properties of Gases

STP

1 mole = 22.4L