VOCAB CHECKLIST: CHECK OFF WHICH WORDS YOU CAN DEFINE
Group A
Single Replacement
%yield
Double Replacement
Coefficient
Synthesis
Arrenhius Acid
Decomposition
Arrenhius Base
Combustion
Bronsted Acid
Mole ratio
Bronsted Base
Stoichiometry
Indicator
Limiting reactant
Amphoteric
Excess reactant
Basic solution
Theoretical yield
Monoprotic acid
Actual yield
Polyprotic acid
Group B
strong base
Energy
weak acid
Enthalpy
weak base
Enthalpy of combustion
Activated Complex
Enthalpy of fusion
Activation Energy
Enthalpy of reaction
Calorie
Enthalpy of vaporization
Calorimeter
Catalyst
Heat
Chemical potential energy
Joule
Collision Theory
Law of conservation energy
Group C
Kinetic Molecular Theory
Insoluble
Boiling pt elevation
Miscible
Colligative property
Molarity
Colloid
Molality
Concentration
Saturated solution
Freezing point
Solubility
depression
Soluble
Immiscible
Solute
Acidic Solution
Conjugate acid
Conjugate Base
End point
Equivalence point
Titration
pH
pOH
salt
strong acid
Specific heat
Surroundings
System
Thermochemistry
Universe
Boyle’s Law
Charle’s Law
Gay-Lussac’s Law
Ideal Gas
Solvation
Solvent
Supersaturated solution
Suspension
Tyndall effect
Unsaturated solution
Vapor pressure lowering
GRAPHS: CHECK OFF GRAPHS THAT YOU CAN EXPLAIN and READ.
____ 1.Heating and Cooling Curves ( label solid, liquid, and gas phases; transition phases; explain energy changes)
____2.Potential Energy Diagram (Endo vs. Exo + main parts: reactant, product, enthalpy, activated
complex, activation energy (forward and reverse)
____3.Solubility Curve (How to tell if a solution is saturated, unsaturated, supersaturate
CHECKLIST fo3 FORMULAS to KNOW: Make flash cards!
___1. Molarity = moles solute/L solution
___2. molality = moles solute/kg solution
___3. M1V1 = M2V2 (dilution)
___3. pH = -log[H+]
___4. pOH = -log [OH-]
___5. pOH + pH = 14
___6. Q = mcΔt
___7. Heat lost = heat gained (heat transfer problems)
___8. % Yield = (actual – theoretical) / theoreticalx100
Practice Problems
I.
If the statement is true, write T. If it is false, write F and change the underlined word to make it true.
1.
Two polar liquids will most likely be immiscible when mixed together.
2.
Shaking and stirring decreases the rate of salvation.
3
A dilute solution contains a small amount of solute relative to the solvent.
4.
Molar solutions are calculated and expressed in grams per liter.
5.
The boiling point elevation is the difference between a solute’s boiling point and a
pure
solvent’s boiling point.
6.
A 1 m solution of a nonelectrolytes solute will have a lesser effect on the
colligative properties of its solution
than than a 1m solution of an electrolyte will have on the colligative properties of its
solutions.
7.
Boiling point depression is the temperature difference between a solution’s and a
pure solvent’s boiling point.
8.
Colloids are heterogeneous mixtures that contain particles between 1 nm and 1000 nm in
diameter.
9.
Enthalpy changes for exothermic reactions are always negative.
10.
A pH greater than 7 indicates a standard solution.
11.
If the pH of a solution is 10, its pOH is 4.
12.
In a neutralization reaction, an acid and a base react to produce an oxide and water.
13.
Gay Lussac’s law states that the volume and Kelvin temperature of a contained gas are directly proportional if
pressure is constant.
II.
Choose the correct answer for the following questions.
14.
After adding a small crystal of copper (II) sulftate to an aqueous solution a slarge amount of copper sulfate precipitate.
Which of the following describes the original solutions?
a.
unsaturated
b. viscous
c. saturated
d. supersaturated
15.
The ability to be separated by paper filtration is a characteristic of which mixture?
a. solution
b. colloids and solution
c. suspension
d. colloids
16.
Which of the following will scatter light?
a. salt water
b. ice tea
c. fog
d. koolaid
17.
Energy flow from a warmer to a cooler object is
a. Specific heat
b. enthalpy
c. heat
d. activation
energy
18.
An insulated device for measuring the heat absorbed or released during a chemical or physical process is called
a.enthalpy of reaction
b . joule
c. valve d. calorimeter
19.
Energy needed to melt one mole of a solid is called
a. molar enthalpy of fusion
b. enthalpy of reaction
c. molar enthalpy of vaporization d. enthalpy of combustion
20.
________________ are the products of a neutralization reaction between a strong
acid and a strong base.
a. salt and water
b. acid and base
c. gas and water
d. hydrogen ions and hydroxide ions
21.
If the pressure of a gas increases while the temperature remains the same, what happens to the volume?
a. it
decreases
b. it increases
c. it stays the same
22.
What is the relationship between temperature and volume at constant pressure?
a. indirect
b. direct
d. no relationship
III.
Fill in the blank
23.
.The solvation of sodium chloride in water occurs because the Na has a ______ charge that
attract to the
_________ in the water and the Cl has a ____ charge that attracts to the
___________ atom in water.
.
24.
25.
26.
27.
28.
Compound A is __________________ and compound B is ____________. I
know this because
_________________________________________________.
The SI unit for heat and energy is ____________________.
In a calorimeter, the water is the ______________________ and the reaction is the system. The two
make up the _______________.
In a reaction, activation energy is the amount of energy needed to ___________________________.
The pOH of a solution is equal to the negative log of the ____________ion concentration
combined
29.
Process A is
___________________(endo/exo?)
because it _______________ heat.
30.
Process B is ______________
because it ________________ heat.
A)
Identify the following equations as Synthesis (s), Decomposition (D), Single Replacement (SR), or
Double Replacement (DR) on the line to the left of the number.
B)
Balance the equation
C)
Write the word equation under the chemical equation.
_____1. N2 + H2  NH3
______________________________________________________________________________________
_____2. CaCO3  CaO + O2
______________________________________________________________________________________
_____3. Se + O2  SeO3
______________________________________________________________________________________
_____4. Sr(NO3)2 + K2 SO4  KNO3 + SrSO4
______________________________________________________________________________________
_____5. C2H4 + O2  CO2 + H2O
_____________________________________________________________________________________
_____6. Cu + HCl  CuCl2 + H2
_____________________________________________________________________________________
IV:
Problem solving:
31.
The solubility of potassium dihydrogen phosphate is 25g/100g at 25 C. What is the molality of this solution?
32.
An exothermic process releases 10,570 Calories. Convert this to kJ.
33.
How much heat has been absorbed by 6500 g of water when its temperature changes from 24.0 C to
28.0 C.
Express in joules.
How many food calories are supplied?
34A.
The
hydrogen ion
concentration of a solution is 9.3x10-12. What is the pH of this solution?
34B.
What is the hydroxide concentration of a solution that has a pH of 4.10?
35.
The hydroxide ion concentration of a solution is 1.9x20-13. What is the pOH, pH and [H+]?
36.
Write a balanced formula equation for the neutralization reaction between nitric acid and solid
caclium hydroxide.
37.
A 66.1mL sample of HCl is titrated to its end point with 33.3 mL of .350 M NaOH, What is the
concentration of the
acid?
38.
A 18.5 mL sample of HCl is titrated to its end point with 25.7 mL of .150 M NaOH. What is the
concentration of the
acid?
39.
The volume and amount of gas are constant in a tire. The initial pressure ande temperature are 1.92
atm and
293K. At what temperature will the gas in the tire have a pressure of 2.25 atm?
40.
Calculate the volume occupied by 7 moles of I2 at STP.
Moles and Stoichiometry
41.
42.
43.
44.
45.
46.
47.
Calculate the number of molecules in 15.7 moles of carbon dioxide.
Calculate the number of moles in 9.22x1023atoms of iron.
Calculate the number of atoms in 3.5 moles of Zn.
What is the mass of 6.89 moles of antimony?
Determine the mass of 0.187 moles of CH4.
Find the % of Aluminum in aluminum oxide.
The composition of acetic acid is 40.00% carbon, 6,71 % hydrogen, and 53.29 % oxygen. Calculate
the empirical formula for acetic acid.
48.
The compound borazine consists of 40.29% boron, 7.51% hydrogen, and 52.20% nitrogen, and its
molar mass is 80.50 g/mol. Find the molecular formula for borazine.
Use the following equation to answer questions 49-52.
4HCl + O2  2 H2O + Cl2
49.
What is the mole: mole ratio of H2O: H2CO3?
50.
How many moles of chlorine gas are formed if 3.5 moles of HCl are used?
51.
How many grams of water are made if 4 moles of HCl are used?
52.
If moles of HCl are used and 4 moles of oxygen, what is the limiting and excess reagent?
The following reaction occurs in plans undergoing photosynthesis:
6CO2 + 6H2O  C6H12O6 + 6O2
53.
How many liters of oxygen are made from 24 moles of CO2?
54.
What is the % yield if the theoretical yield is 25 grams and the actual is 20 grams?
Grams
Of Compound
x
x
1mole
MolarMass
MolarMass
1mole
6.02 x1023
x
1mole
# particles –
molecules,formula
units,ions,atoms
Grams of
element
atomicMass
x
1mole
x
MOLES
x
x
1mole
6.02 x10 23
xx
1mole
atomicMass
22.4 L
1mole
1mole
22.4 L
Liters
Of Gas