Download 2014-15 FINAL REVIEW Nomenclature: Chemical Name Chemical

2014-15 FINAL REVIEW
Nomenclature:
Chemical Name
Chemical Formula
NH4OH
BaCl2
magnesium chlorate
KC2H3O2
chromium(II) sulfate
Cu(NO2)2
silver nitrate
Na2O
copper(II) chloride
sodium chromate
Balancing Equations:
1. ____HCl + ____Ba(OH)2  ____BaCl2 + ____H2O
2. ____H3PO4 + ____NaOH  ____Na3PO4 + ____H2O
3. ____Pb(NO3)2 + ____KI  ____ PbI2 + ____KNO3
4. ____CuO + ____NH3  ____N2 + ____Cu + ____H2O
5. ____C2H5OH + ____O2  ____CO2 + ____H2O
Empirical/Molecular Formulas:
Empirical Formula
C2H6O2
a)
X39Y13
b)
Molecular Formula
A compound with an empirical formula of
C2OH4 and a molar mass of 88
grams/mole.
A compound with an empirical formula of
C4H4O and a molar mass of 136
grams/mole.
c)
d)
Gas Laws:
1. A child has a toy balloon with a volume of 1.80 liters. The temperature of the balloon when it was filled was
200 C and the pressure was 1.00 atm. If the child were to let go of the balloon and it rose 3 kilometers into
the sky where the pressure is 0.667 atm and the temperature is -100 C, what would the new volume of the
balloon be?
2. If divers rise too quickly from a deep dive, they get a condition called “the bends” which is caused by the
expansion of very small nitrogen bubbles in the blood due to decreased pressure. If the initial volume of
the bubbles in a diver’s blood is 15 mL and the initial pressure is 12.75 atm, what is the volume of the
bubbles when the diver has surfaced to 1.00 atm pressure?
3. It is not safe to put aerosol canisters in a campfire, because the pressure inside the canisters gets very high
and they can explode. If I have a 1.0 liter canister that holds 2 moles of gas, and the campfire temperature
is 14000 C, what is the pressure inside the canister?
4. How many moles of gas are in a 30 liter scuba canister if the temperature of the canister is 300 K and the
pressure is 200 atmospheres?
5. What’s the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of
nitrogen, and 1 mole of hydrogen and has a total pressure of 1.05 atm?
Moles & Stoich:
1. Using the following equation: 2 NaOH + H2SO4  2 H2O + Na2SO4
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and
you have an excess of sulfuric acid (H2SO4)?
2. Using the following equation: Pb(SO4)2 + 4 LiNO3  Pb(NO3)4 + 2 Li2SO4
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you
have an adequate amount of lead (IV) sulfate to do the reaction?
Volume & Stoich:
1. A sample of propane gas, C3H8, contains 3.50x1022 molecules at STP.
(a) How many moles are in this sample?
(c) What is the volume of the sample?
(b) What is the mass of this sample?
(d) How many hydrogen atoms are in this
sample (not in moles)?
2. Given the following reaction: 4 Fe (s) + 3 O2 (g) --> 2 Fe2O3 (s)
(a) If 37.5 grams of Fe2O3 is produced, find the moles of Fe that react.
(b) If 37.5 grams of Fe2O3 is produced, find the volume of O2 that reacts at STP.
(c) If 37.5 grams of Fe2O3 is produced, find the volume of O2 that reacts at 1.1 atm and 25°C.
(d) What mass of Fe is needed to react with 13.0 L of oxygen at 733 mmHg and 10°C?
3. How many liters of hydrogen can be produced by reacting 4.0 g of aluminum with excess hydrochloric acid
(a) if the hydrogen is collected at STP
(b) if the hydrogen is collected at 0.92 atm and 30°C?
Net Ionic Equations:
1. strontium bromide(aq) + potassium sulfate(aq)  strontium sulfate(s) + potassium bromide(aq)
2. Ni(NO3)3 (aq) + KBr(aq) 
3. cobalt(III)bromide + potassium sulfide 
Concentration & Stoich:
1. What is the molarity of 5.00 g of NaOH in 750.0 mL of solution?
2. What weight (in grams) of H2SO4 would be needed to make 750.0 mL of 2.00 M solution?
3.
If you mix 200 ml of 0.100 M Pb(NO3)2 and 300 ml of 0.200 M MgCl2, how much PbCl2 precipitate will you
form?
4. How many liters of a 0.75 M solution of Ca(NO3)2 will be required to react with 148 g of Na2CO3?
__ Ca(NO3)2 + __ Na2CO3  __ CaCO3 + __ NaNO3
5. 100.0 mL of 0.200M aqueous potassium hydroxide is mixed with 100.0mL of 0.200M aqueous magnesium
nitrate. What mass of magnesium hydroxide is formed? What is/are the concentration of any ions
remaining in the solution?
Heat of Reaction:
1. Hg has a specific heat of 0.139 J/goC. How much heat is required to raise the temperature of a 22.80 g
sample from 16.1oC to 32.5oC?
2. Some water is heated from 10.0oC to 50.0oC. During the process, 50.0 kiloJoules of heat is added to the
water. What is the mass (grams) of water heated?
3. The specific heats of 3 different substances are listed as:
carbon tetrachloride: 0.856 J/goC
benzene: 1.74 J/goC
acetic acid: 2.05 J/goC
A chemistry student finds that 1.47 kJ of heat raised the temperature of 19.70 g of an unknown substance
by 36.4oC. Which of the three substances listed is the unknown substance?
4. What final temperature will 120.00 g of benzene at 7.00oC have after it absorbs 2.20 kJ of heat? The Cp of
benzene is 1.74 J/goC.
Equilibrium:
1. List 3 stressors that would shift this reaction to the left:
CH4(g) + 2H2S(g) ↔ CS2(g) + 4H2(g)
2. What would happen to the position of the equilibrium when the following changes are made to the
equilibrium system below?
2SO3(g) ↔ 2SO2(g) + O2(g)
a. Sulfur dioxide is added to the system.
b. Sulfur trioxide is removed from the system.
c. Oxygen is added to the system.
3. Write the equilibrium expression for the following reactions:
N2 (g) + 3 H2 (g)  2 NH3 (g)
I2 (s) + Cl2 (g)  2 ICl (g)
NO2 (g)  NO (g) + ½ O2 (g)
4. The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25C of 1.8 x 10-5. The reaction is
CH3COOH (aq)  CH3COO- (aq) + H+ (aq)
If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO- is 8.1 x
10-3 moles in the same 0.500 L, calculate [H+] for the reaction.
ANSWER KEY
Nomenclature:
Chemical Name
Ammonium hydroxide
magnesium chlorate
Chemical Formula
Mg(ClO3)2
Barium chloride
sodium chromate
Na2CrO4
KC2H3O2
Potassium acetate
chromium(II) sulfate
CrSO4
Cu(NO2)2
Copper (II) nitrite
silver nitrate
AgNO3
Na2O
Sodium oxide
copper(II) chloride
CuCl2
NH4OH
BaCl2
Balancing Equations:
1. _2_HCl + _1_Ba(OH)2  _1_BaCl2 + _2_H2O
2. _1_H3PO4 + _3_NaOH  _1_Na3PO4 + _3_H2O
3. _1_Pb(NO3)2 + _2_KI  _1_ PbI2 + _2_KNO3
4. _3_CuO + _2_NH3  _1_N2 + _3_Cu + _3_H2O
5. _1_C2H5OH + _3_O2  _2_CO2 + _3_H2O
Empirical/Molecular Formulas:
a) CH3O
b) X3Y
c) C4O2H8
d) C8H8O2
Gas Laws:
1. 2.42 L
2. 191 mL
3. 274.5 atm
4. 243.7 moles
5. .583 atm
Moles & Stoich:
1. 355.3 g
2. 313.6 g
Volume & Stoich:
1. A) .0581 mol
B) 2.56 g
C) 1.30 L
D) 2.80 x 1023
2. A) 0.469 mol
B) 7.88 L
C) 7.82 L
D) 40.2 g
3. A) 4398 L B) 6.01 L
Net Ionic Equations:
1. Molecular: SrBr2 (aq) + K2SO4 (aq)  SrSO4 (s) + 2 KBr (aq)
Total Ionic: Sr2+ (aq) + 2 Br¯ (aq) + 2 K+ (aq) + SO42- (aq)  SrSO4 (s) + 2 K+ (aq) + 2 Br¯ (aq)
Net Ionic: Sr2+ (aq) + SO42- (aq)  SrSO4 (s)
2. Molecular: Ni(NO3)3 (aq) + 3 KBr (aq)  NiBr3 (aq) + 3 KNO3 (aq)
Total Ionic: Ni3+ (aq) + 3 NO3¯ (aq) + 3 K+ (aq) + 3 Br¯ (aq)  Ni3+ (aq) + 3 NO3¯ (aq) + 3 K+ (aq) + 3 Br¯ (aq)
Net Ionic: No reaction
3. Molecular: 2 CoBr3 (aq) + 3 K2S(aq)  Co2S3 (s) + 6 KBr (aq)
Total Ionic: 2 Co3+ (aq) + 6 Br¯ (aq) + 6 K+ (aq) + 3 S2- (aq)  Co2S3 (s) + 6 K+ (aq) + 6 Br¯ (aq)
Net Ionic: 2 Co3+ (aq) + 3 S2- (aq)  Co2S3 (s)
Concentration & Stoich:
Heat of Reaction:
1. 0.167 M
1. 52.0 J
2. 147 g
2. 299 g
3. 5.55 g
3. Acetic acid
4. 1.86 L
4. 17.5 °C
5. 0.583g [K+]= 0.1 M [Mg2+] = 0.05M
Equilibrium:
1. There are many answers: a) Decrease the [dihydrogen sulfide]; b) Increase the pressure on the system; c)
Increase the [carbon disulfide]; d) Decrease the [methane].
2. A) Shift left
B) Shift left
C) Shift left
3. K = [NH3]2
K = [ICl]2
K = _[NO] [O2]1/2
[N2] [H2]3
[Cl2]
[NO2]
4. [H+] = 1.0 x 10-3 M