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Section 1

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Boyle's Law

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Chemistry Science

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Date created

Mar 1, 2020

Cards (38)

Section 1

(38 cards)

Boyle's Law

Front

A principle that describes the relationship between the pressure and volume of a gas at constant temperature expressed as the equation P1V1=P2V2

Back

Celsius

Front

0°= freezing and 100°= boiling

Back

Kinetic Molecular Theory

Front

the theory that all matter is composed of particles (atoms and molecules) moving constantly in random directions. Properties include: •move rapidly and randomly •have no volume •no retractive or repulsive forces between particles •all collisions are elastic •average kinetic energy or particles are directly proportional to the temperature •when they collide they do not gain or lose energy

Back

Pressure

Front

the amount of force exerted per unit area of a surface

Back

Formula Mass

Front

Sum of the atomic weights in an empirical formula.

Back

Avogadro's Law

Front

the number of moles of gas varies directly with the volume of a gas at constant temperature and pressure

Back

atmospheres

Front

a constant representing the force exerted by the Earth's atmosphere on 1 square meter at sea level.

Back

Actual Yield

Front

A measured quantity of the actual amount of product produced during a chemical reaction

Back

Effusion

Front

A process by which gas particles pass through a tiny opening

Back

Decomposition

Front

A compound is broken down into simpler compounds, or all the way down to the simper elements that make it up.

Back

Single Replacement

Front

One element that starts out by itself replaces another element in the compound, kicking it out.

Back

STP (standard temperature and pressure)

Front

These units are shown as 0°C or 273 Kelvin(k) for temperature and 1 atm or 760 torr for pressure.

Back

Temperature

Front

A measure of the average energy of motion of the particles of a substance. Also measure how hot or cold something is usually in C or F.

Back

Gay-Lussac's Law

Front

aka the pressure law. the pressure of a gas varies directly with the temperature at a constant volume; P1/T1=P2/T2

Back

psi

Front

pounds per square inch

Back

Diffusion

Front

Movement of molecules from an area of higher concentration to an area of lower concentration.

Back

Synthesis

Front

A compound is made from similar materials.

Back

Empirical Formula

Front

Notation showing the lowest whole number ratio of atoms in a compound.

Back

Double Replacement

Front

The positive and negative ions in two compounds switch places.

Back

MmHg

Front

Millimeter of Mercury. Non SI unit of pressure. = 1 Torr/ 760 atm.

Back

Molar Volume

Front

Volume occupied by one mole of a substance.

Back

Celsius

Front

The temperature scale on which water freezes at 0 degrees and boils at 100 degrees

Back

Charles' Law

Front

the temperature of a gas varies directly with volume at constant pressure expressed as the equation V1/T1=V2/T2

Back

Percent Yield

Front

the ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; shown as actual yield/theoretical yield x 100

Back

Barometer

Front

Used to measure atmospheric pressure.

Back

Avogadro's Principle

Front

equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

Back

Mole

Front

SI unit used to describe the # of particles of a substance that are present. 1 mole= 6.02x10^23

Back

Kelvin

Front

The SI base unit of temperature

Back

1 Torr equals..

Front

1 mmHg

Back

Ideal Gas Law

Front

the relationship which describes the behavior of a gas in terms of temperature, pressure, volume and number of moles express as Pv=nrt.

Back

760 mmHg equals..

Front

14.7 psi and 1 atm

Back

Molecular Mass

Front

Sum of atomic masses of molecular compounds.

Back

Kelvin

Front

SI base unit of temperature, k.

Back

Combustion

Front

A compound containing carbon and hydrogen (sometimes oxygen) combines with oxygen gas to produce carbon dioxide and water.

Back

Theoretical Yield

Front

a quantity that is always cslculated and shoes the theoretical amount of a product that could be produced in an ideal chemical reaction in which there is a complete conversion of reactants to products

Back

Graham's Law

Front

the rate of effusion of a gas is inversely proportional to the square root of its molar mass

Back

Combined Gas Law

Front

can be used to determine the pressure, volume, or temperature of gases and can be expressed as P1V1/T1=P2V2/T2

Back

Dalton's Law of Partial Pressure

Front

the total pressure of a mixture of gases is the sum of the partial pressures of the gases contained within that mixture

Back