Chem Exam 2

Front 1

How do you convert g —> mol ?

Back 1

Divide by molar mass.

Front 2

How do you convert from mol —> g ?

Back 2

Multiply by molar mass.

Front 3

How do you convert from mol —> particles ?

Back 3

Multiply by Avagadro’s number.

Front 4

How do you convert from particles —> mol ?

Back 4

Divide by Avagadro’s number.

Front 5

What is Avagadro’s number?

Back 5

6.022 x 10^23

Front 6

________ is the number of entities composing one mole.

Back 6

Avogadro’s number.

Front 7

__________ is the amount of substance containing the same number of discrete entities as the number of atoms in a sample of pure 12C weighing exactly 12 g.

Back 7

The mole.

Front 8

Avogadro’s number is a(n) ______ number.

Back 8

Exact.

Front 9

What is meant by Avogadro’s number being an exact number?

Back 9

It does not have a set number of significant figures. It is an infinite number.

Front 10

___________ is the mass of one mol of anything.

Back 10

Molar Mass.

Front 11

g/mol is the unit for ___________.

Back 11

Molar mass.

Front 12

The empirical formula of a compound can be derived from...?

Back 12

The masses of all elements in the sample.

Front 13

_______ formulas give the lowest whole number ratio of atoms in a molecule.

Back 13

Empirical formula‘s.

Front 14

_______ formulas give the total number of atoms in a molecule.

Back 14

Molecular formulas.

Front 15

_______ formulas give the total number of atoms in a molecule.

Back 15

Molecular formulas.

Front 16

_______ compounds are always written as the empirical formula.

Back 16

Ionic compounds.

Front 17

________ : the relative number of particles in a given volume of solution.

Back 17

Concentration.

Front 18

________ : the relative number of particles in a given volume of solution.

Back 18

Concentration.

Front 19

________ : the component of a solution in the greatest quantity.

Back 19

Solvent.

Front 20

_______: the component of a solution which is dispersed in the solvent.

Back 20

Solute.

Front 21

Solutions where water is the solvent are called...

Back 21

Aqueous solutions.

Front 22

What is the formula for molarity?

Back 22

M = moles solute / liters of solution

Front 23

Chemical reactions take place on a _________, the most common unit of concentration for solutions is _______.

Back 23

Molar basis ; molarity.

Front 24

_______ is the process of making a solution less concentrated by adding more solvent.

Back 24

Dilution.

Front 25

Dilution is the process of making a _____ less concentrated by adding more ______.

Back 25

Solution ; Solvent.

Front 26

What is the formula to determine the concentration of a diluted solution?

Back 26

(C1)(V1) = (C2)(V2)

Front 27

____________ is the ratio of a solute’s mass to the mass of the solution, expressed as a percentage.

Back 27

Mass percentage.

Front 28

___________ is the ratio of a solute’s volume to the volume of the solution, expressed as a percentage.

Back 28

Volume percentage.

Front 29

What is the mass percentage formula?

Back 29

(Mass of solute/mass of solution) x 100 = mass/mass percentage.

Front 30

What is the formula for volume percentage?

Back 30

(Volume of solute/volume of solution) x 100 = volume/volume percentage

Front 31

___________ is the ratio of a solute’s mass to the solution’s volume, expressed as a percentage.

Back 31

Mass/volume percentage.

Front 32

What is the mass/volume percentage formula?

Back 32

Back (Definition)

Front 33

Mixed percent units (“mass/volume percentage”) are usually seen in...

Back 33

Healthcare.

Front 34

PPM stands for ______ and can be identified by 10^___.

Back 34

Parts per MILLION. ; 10^6.

Front 35

PPB stands for _______ and can be identified by 10^___.

Back 35

Parts per BILLION. ; 10^9.

Front 36

T/F: Parts per million (ppm) and parts per billion (ppb) are units calculated in a manner close to percentage (part per hundred).

Back 36

True.

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