Ch 7-16
1. The reaction between copper(II) sulfate and zinc, involves the transfer of electrons from ________________.
a) zinc to copper(II)
b) sulfate to zinc
c) sulfate to copper(II)
d) copper(II) to zinc
2. "Lead trees" are formed in the reaction between zinc and lead(II) nitrate, which is an example of a(n)
a) combustion reaction
b) precipitation reaction
c) acid-base reaction
d) oxidation reduction reaction
3. ____________ precipitates from the reaction between silver nitrate and sodium chloride.
a) Sodium chloride
b) Sodium nitrate
c) Silver chloride
d) Silver nitrate
4. Silver ions forms an insoluble salt with __________
a) potassium ions
b) chromate ions
c) ammonium ions
d) nitrate ions
5. The crystallization of sodium acetate from a saturated solution is a ______________.
a) physical process
b) chemical process
c) explosive event
d) rare event
6. Zinc reacts in aqueous acid solutions to produce ___________.
a) oxygen gas
b) hydrogen gas
c) zinc metal
d) chlorine gas
7. When a current is supplied water is electrolyzed to give
a) hydroxide ions
b) hydrogen ions
c) hydrogen and oxygen gas
d) hydride ion
8. Depositing soot on a surface above a burning candle is an example of a
a) chemical process
b) combustion reaction
c) physical process
d) oxidation-reduction reaction
9. When a droplet of concentrated hydrochloric acid is exposed to ammonia gas, the resulting smoke consists of
a) hydrogen chloride
b) nitrogen gas
c) sodium chloride
d) chlorine gas
e) ammonium chloride
Ch 7-5
1. Certain commercial chemical heat packs involve the precipitation of solid sodium acetate from a supersaturated solution of the dissolved salt. This is illustrated by the following equation:
NaC2H3O2(aq) → NaC2H3O2(s) + heat
This is an example of a(n)
a) neutralization reaction
b) oxidation reaction
c) chemical change
d) physical change
2. Which of the following chemical equations represents the reaction between lead(II) nitrate and sodium chloride?
a) Pb(NO3)2(aq) + NaCl(aq) → PbCl2(s) + NaNO3(aq)
b) Pb(NO3)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaNO3(aq)
c) Pb(NO3)2(s) + 2 NaCl(s) → PbCl2(aq) + 2 NaNO3(aq)
d) PbNO3(aq) + 2 NaCl(aq) →PbCl(s) + 2 NaNO3(aq)
3. Which of the following reactions is a neutralization reaction?
H2(g)+F2(g)→2HF(g)
a) HCl(aq) + NaOH(aq) →NaCl(aq) + H2O(l)
b) C6H12O6(s)+O2(g)→CO2(g)+H2O(g)
c) H2(g) + O2(aq) → H2O(g)
d) AgNO3(aq)+ NaI(aq) →AgI(s) + NaNO3 (aq)
4. Which of the following reactions would you expect to generate the most heat energy on a molar basis?
a) HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)
b) 2NaOH(aq)+MgCl2(aq)→2NaCl(aq)+Mg(OH)2(s)
c) 3CuO(s) + 2Al(s) → 3Cu(s) + Al2O3(s)
d) AgNO3(aq)+ NaI(aq) →AgI(s) + NaNO3(aq)
Ch 9
1. Before completing any stoichiometry problem you must balance the chemical equation. Give the balanced equation for the reaction of carbon dioxide gas with lithium hydroxide to give lithium carbonate and water.
a) 2CO2(g) + 2LiOH(s) → 2Li2CO3(aq) + H2O(l)
b) 2CO2(g) + 4LiOH(s) → 2Li2CO3(aq) + 2H2O(l)
c) CO2(g) + 2LiOH(s) → Li2CO3(aq) + H2O(l)
d) 2CO2(g) + 4LiOH(s) → 2Li2CO3(aq) + H2O(l)
2. After allowing for a substantial safety margin, it has been determine that the astronauts may generate as much as 1.00 x 103 moles of carbon dioxide. How many grams of lithium hydroxide will be needed to react with this quantity of CO2?
a) 1.20 kg
b) 12.0 kg
c) 4.78 kg
d) 47.8 kg
e) 2.39 kg
f) 23.9 kg
3. In one scenario, it is calculated the astronauts may generate as much as 100.0 moles of carbon dioxide. In addition, it is determined that the scrubbers are only 80% efficient. Under these circumstances, how many grams of lithium hydroxide are required to ensure complete remove the carbon dioxide?
a) 8.60 kg
b) 2.99 kg
c) 3.83 kg
d) 5.98 kg
4. The astronauts are to build makeshift scrubbers to accommodate the canisters from the Command Module. The scrubbers must be able to handle the water generated when LiOH reacts completely with carbon dioxide. How much water will be generated when a single 12.0 kg canister of lithium hydroxide reacts completely with excess carbon dioxide? Assume 100 percent efficiency.
a) 4.51 kg
b) 9.03 kg
c) 7.97 kg
d) 108 kg
Ch 10-11
1. From the heat capacity equation we can see that we will need the mass of the beverage. Assume that the beverage is water at 25°C.
Given that we have 8.0 fluid ounces, what is the mass of the beverage in grams?
l There are 28.413 mL of water in 1 fluid ounce
l The density of water is 1.0 grams per 1.0 mL at 25°C
a) 230 g
b) 290 g
c) 3.6 g
d) 28 g
2. How many moles of calcium oxide must be present to produce the necessary amount of heat energy to warm the beverage?
CaO (s) + H2O (l) → Ca(OH)2 (aq) ΔH = -63.7 kJ/mol
a) 0.58 moles
b) 2300 moles
c) 33 moles
d) 1 mole
3. How many grams of calcium oxide do we need for this reaction?
a) 56 g
b) 0.010 g
c) 33 g
d) 130 kg
4. How many milliliters of water are needed?
a) 580 mL
b) 131 mL
c) 10.0 mL
d) 667 mL
5. Suppose you used a thermite reaction to heat the beverage. How many grams of iron(III) oxide would be needed? (Molar mass: 159.69 g/mol)
Fe2O3 + 2 Al → 2 Fe + Al2O3 ΔH = -547.5 kJ/mol
a) 20 g
b) 115 g
c) 11 g
d) 591 g
Ch 11-5(1)
1. When a mixture containing a pure metal salt is heated to very high temperature light is emitted as a(n) _________________
a) emission spectrum
b) invisible spectrum
c) continuous spectrum
d) absorption spectrum
2. Which of the following colors is due to photons with the greatest energy?
a) Purplr
b) Orange
c) Red
d) Green
e) Blue
f) Yellow
Ch 11-5(2)
1. In terms of the classic "flame triangle" which of the following serves as "oxygen" in the black powder used to launch fireworks:
a) metal salts
b) carbon
c) potassium nitrate
d) Sulfur
2. The carbon and sulfur in black powder react with a strong oxidizing agent to produce _____________
a) potassium nitrate and heat
b) sulfur, carbon and heat
c) carbon dioxide, sulfur dioxide and heat
d) nitrogen, oxygen and heat
3. To generate sufficient energy needed to induce the electronic transitions in the metal salts that result in the colorful displays of light one needs to employ highly energetic oxidation reduction reactions. Which of the following reactions is likely to generate sufficient energy? (there may be more than one answer)
a) HCl(aq) + NaOH(aq) → NaCl(aq) +H2O(l)
b) 3KClO3(s) + C6H12O6(s) → 3KCl(s) + 6H2O(g) + 6CO2(g)
c) Fe2O3(s) + 2 Al(s) → 2 Fe(s) + Al2O3(s) a thermite reaction
d) NaCl(aq) + AgNO3(aq) → AgCl(s) +NaNO3(aq)
4. Which ingredient(s) served as the fuel source in Captain Kirk's "cannon"?
a) carbon
b) sulfur
c) saltpeter
d) carbon and sulfur
Ch 13
1. For your calculations, assume that the nitrogen gas is produced under conditions of standard temperature and pressure (STP). What is STP?
a) 0 K and 101.325 kPa
b) 273 K and 1 atm
c) 25°C and 760 torr
d) 32°F and 1.01325 Pa
2. How many moles of nitrogen gas must be produced to fill a volume of 65.0 Liters at STP?
Use PV=nRT and solve for n
a) 2.56 moles
b) 2.78 moles
c) 3.01 moles
d) 2.90 moles
3. What is the molar mass of sodium azide?
a) 63.1 g/mole
b) 120.0 g/mole
c) 65.00 g/mole
d) 89.3 g/mole
4. What is the molar mass of elemental nitrogen?
a) 14.0 g/mole
b) 16.0 g/mole
c) 12.0 g/mole
d) 28.0 g/mole
5. Why is it necessary to oxidize the sodium metal that is produced in the decomposition of sodium azide?
a) sodium is a reactive metal
b) sodium is a volatile gas that adds significant volume
c) sodium is an ionic plasma that adds significant volume
d) sodium is a strong strong oxidizing agent
6. Which of the following chemical equations describes the reaction of sodium metal with iron(III) oxide?
a) 2Na(s) +FeO(s) → Na2O(s) + Fe(s)
b) 6Na(s) + Fe2O3(s) → 3Na2O(s) + Fe(s)
c) 3Na(s) + Fe2O3(s) → 3Na2O(s) + 2Fe(s)
d) 6Na(s) + Fe2O3(s) → 3Na2O(s) + 2Fe(s)