2nd Semester Exam Review
(Turn in on exam day)
Name _______________________________
Sample Questions:
1. A cup of liquid water loses energy to its environment. Which phase change might occur as a result of this loss of energy?
a. Sublimation
b. freezing
c. boiling
d. melting
2.
A chemical reaction produces heat as the reaction progresses. Which statement is correct?
a. A catalyst was used to produce the heat.
b. The products had more energy than the reactants.
c. An inhibitor was used to produce the heat.
d. The reactants had more energy than the products.
3. Which of these changes produces the greatest increase in entropy?
a. CO2(g)  CO2(s)
b. H2O(g)  H2O(l)
c. 2Mg(s) + O2(g)  2MgO(s)
d. CaCO3(s)  CaO(s) + CO2(g)
4.
Given the balanced equation: 4Fe(s) + 3O2(g)  2Fe2O3(s) + 1640 kJ Which phrase best describes this reaction?
a. endothermic with H = +1640 kJ
b. exothermic with H = -1640 kJ
c. endothermic with H = -1640 kJ
d. exothermic with H = +1640 kJ
5.
Given the balanced equation: I(s) + energy  I (g) As a sample of I (s) sublimes to I(g), the entropy of the sample:
a. decreases because the particles are less randomly arranged.
b. increases because the particles are more randomly arranged.
c. decreases because the particles are more randomly arranged.
d. increases because the particles are less randomly arranged.
6.
Systems in nature tend to undergo changes toward:
a. lower energy and higher entropy.
B. higher energy and higher entropy.
c. higher energy and lower entropy.
D. lower energy and lower entropy.
7.
Given the balanced equation: KNO3(s) + 34.89 kJ  K+(aq) + NO3- (aq) Which statement best describes this process?
a. It is endothermic and entropy decreases.
b. It is endothermic and entropy increases.
c. It is exothermic and entropy decreases.
d. It is exothermic and entropy increases.
8.
Given the following chemical equation: KC1O3  KC1 +O2. Which number would appear in front of KC1 in the balanced
chemical equation?
a. 1
b. 2
c. 3
d. 4
9.
Given the chemical equation: X + Cl2  C2H5Cl + HC1. Which molecule is represented by the letter X?
a. C2H6
b. C3H8
c. C2H4
d. C3H6
10. Write the balanced equation for the neutralization reaction between hydrosulfuric acid and Iron II hydroxide:
a.
Add the labels (s) and (aq) above:
b.
Which substance is the proton donor in the reaction?
c.
What is the % composition of iron in the product, iron II sulfide?
d.
How many grams of acid are needed to produce 10.0g of the salt?
Which acid/base theory tells us this?
11. Write the balanced equation for the synthesis reaction between hydrogen and oxygen that produces water:
a.
How many grams of water are produced if you started with 25.0L of hydrogen gas?
b.
How many molecules of oxygen were consumed when reacting with this amount of hydrogen?
Refer to the graph for the following questions:
12. Which unknown is most likely a gas?
13. Which unknown is saturated with 40g at 75 °C?
14. Which unknown is unsaturated with 60g at 80 °C?
15. Which unknown is Supersaturated with less than 5g at 80°C?
16. How many grams of unknown A can dissolve at 80°C?
17. How many grams of solute will crystallize out of solution if a
saturated solution of B at 90 °C is cooled to 30°C?
18. What solvent was used in this situation?
2nd Semester Exam Review II(Turn in on exam day)
Name: ______________________
Gas Laws:
1. How do you covert temperature from Celsius to Kelvin?
2. What the ideal gas law?
Combined gas law?
Boyle’s?
Gay-Lussac?
Charles?
3. What is the final volume of a 300.0 mL gas sample that is subjected to a temperature change from 0.0 °C to
30.0 °C and a pressure change from 760.0 mm Hg to 260.0 mm Hg?
*1st predict: Do you think the volume will increase or decrease?_________
4. 15.2 grams of nitrogen gas reacts with excess hydrogen gas at STP to form ammonia gas (NH3). What
volume of ammonia gas is formed?
Light and Photons, Oxidation/Reduction, and other misc. topics:
1. If a reaction is ENDOthermic and entropy is DECREASING, we know that it is ______________.
a. not spontaneous
b. spontaneous
2. Define kinetics:
Define Thermodynamics:
3. Given the equation: 2 Al + 3 Cu2+ → 2 Al3+ + 3 Cu, The OXIDATION half-reaction is:
4. What is Hess’s Law?
5. Is the reaction to the right endo or exothermic?
a. Endothermic
b. exothermic
6. According to the diagram, the ∆H is about:
a. 90kJ b. 60kJ
c. 30kJ
d. -60kJ
7. What is the Ea according to the diagram?
a. 90kJ b. 60kJ
c. 30kJ
d. -60kJ
8.
e. -30kJ
e. -30kJ
Given the balanced equation representing the reaction occurring in a voltaic
cell: Zn(s) + Pb2+(aq)  Zn2+(aq) + Pb(s)
In the completed external circuit, the electrons flow from ___________ to _____________.
Types of Reactions:
1. Single replacement reaction of sodium reacting with silver oxide
(Write the products then balance)
2. propane (C3H8) reacts with oxygen
(Write the products then balance)
Reaction type:___________

Is this reaction exo or endothermic?
3. sodium bicarbonate is heated to produce carbon dioxide, water and sodium carbonate.
(Write the products then balance)
Reaction type:___________
Does entropy increase or decrease?
Is this reaction exo or endothermic?
Formulas and Naming of Compounds and Molecules:
1.
Write the formula for the following:
e. oxygen gas
a. Silver chromate
f.
b. Gold foil
g. nitrogen gas
c. Oxygen gas
h. iron (II) oxide
d. tetraphosphorus triselenide
i.
aluminum acetate
calcium pellets
2. Write the name for the following:
a. Fe2O3
b. Al(OH)3
c. C2Br6
3. Write the formulas for the following acids:
a. Hydrosulfuric
b. Sulfuric
c.
Sulfurous
*There will also be a couple of light/photon problems using our E=hf and c=fλ
d. KNO3
e. PH3