Chemistry (Semester 2) Final Exam Questions

a statement that uses chemical formulas to show the identities and relative amounts of the substances of a chemical reaction

chemical equation

a starting substance in a chemical reaction

reactant

as the temperature of a gas increases, the pressure also increases if the volume remains constant

gay lussacs law

liquids are less fluid than gases because

their intramolectular forces are stronger

identify the type of chemical reaction shown here- 2C2H6(g) + 7O2 (g) ---> 4CO2(g) + 6H2O(l)

combustion

identify the type of chemical reaction shown here- CO2(g) +CaO(s) ---> CaCO3(s)

synthesis

at standard temperature and pressure, one mole of any gas occupies _________ of space

22.4L

identify the type of chemical reaction shown here, 2H20(l) ---> 2H20(l) + O2(g)

decomposition

when the volume of a gas is increased, what happens to the pressure within the gas if the volume is constant

pressure decreases

one atmosphere of pressure is equivalent to

101.3kPa

identify the type of chemical reaction shown here- Mg(s) + 2AgNO3(aq) ---> 2Ag(s) + Mg(NO3)2(aq)

single replacement

a reaction in which a compound breaks down into two or more elements of new compounds

decomposition reaction

STP is defined as

0K, 101.3kPa

a solid produced during a chemical reaction in a solution

precipitate

the process by which the atoms of one or more substances are rearranged to form different substances

chemical reaction

a reaction in which two or more substances react to produce a single product

synthesis reaction

an equation that shows all of the articles in solution as they actually exist

complete ionic equation

an equation that includes only the particles that participate in the reaction

net ionic equation

an ion that is present but does not participate in a reaction

spectator ion

a substance formed during a chemical reaction

product

(?) according to the kinetic molecular theory, the particles which make up a gas

are in constant random motion

gases are typically less dense than solids because

of the distance between its particles

(?) the rate at which a gas diffuses is not affected by

the sped of its particles

according to graham's law of effusion, the rate of effusion for a gas is

inversely related to the square root of the molar mass of the gas

a reaction involving the exchange of positive ions between two compounds dissolved in water

double replacement reaction

when a gas is compressed, its density

increases

at elevations above sea level, such as here in Illinois, atmospheric pressure is generally

below one atmosphere

the device used to measure atmospheric pressure is the

barometer

a number written in front of a chemical symbol

coefficient

hydrogen bonds are types of

intermolecular forces

which intermolecular forces would exist between molecules of methane, CH4

hydrogen bonds

the temperature at which the forces which hold particles in a crystal lattice are broken is called

melting point

the reactant at which determines the actual amount of product formed during a chemical change is the

limiting reactant

which of the following molecules would be considered non polar? H20, CO2, HCl, CH3Cl, or NH3

CO3

identify the type of chemical reaction shown here- 2KOH(aq) + H2SO4(aq) ---> K2SO4(aq)

combustion

the mathematical expression P1V1=P2V2 corresponds directly to

boyle's law

the ideal gas law would be mathematically expressed

PV=nRT

the water found within a hydrated crystal

water of hydration

the mass of one mole of anything

molar mass

a formula used to represent a group of covalently bonded atoms

empirical formula

the percent by mass of each element in a compound

percent composition

lacking or without water

anhydrous

6.02x10 (to the 23rd)

avogadro's number

the formula with the smallest whole number mole ration of elements

molecular formula

6.02x10 (to the 23rd) particles

mole

the particle which makes up a substance

representative particles

a compound that has a specific number of water molecules bound to its atoms

hydrated crystal

when gases change directly into solids

deposition

the amount of force exerted over a certain area

pressure

the weakest of the intermolecular forces

hydrogen bonds

a unit of pressure

kilopascal (kPa)

describes the relationships between the pressures of different gases within a mixture

dalton's law

change of a liquid into a gas

vaporization

the intermolecular forces which exist between molecules which have positive and negative ends

dipole dipole forces

the change of a gas into a liquid

condensation

describes relationship between rates of effusion of gases

graham's law

the forces which exist within molecule

intermolecular forces

the change of a solid directly into a gas without melting

sublimation

the forces which exist between molecules

dispersion forces

when a substance will not dissolve in another

insoluble

when two or more liquids are soluble in one another

miscible

a solution which contains less than the maximum amount of solute

unsaturated solution

(?) solutions which contain more solute than normal

solvation

(?) the maximum amount of solute which can dissolve into a solvent

solubility

the substance into which another substance dissolves

solvent

a solution which contains the maximum amount of solute possible

saturated solution

when a substance is able to dissolve into another

soluble

the overall energy change that occurs during solvation

heat of solution

the substance which dissolves into another

solute

any solution in which the solvent is water

aqueous

a homogenous mixture in which one or more substances is dissolved in another

solution

inability of two liquids to mix with one another

immiscible