MC_Chem1A_Sp08_LabQuiz2

Multiple Choice
Identify the choice that best completes the statement or answers the question.

____	1.	When methanol undergoes complete combustion, the products are carbon dioxide and water.

__ CH3OH(l) + __ O2(g) ® __ CO2(g) + __ H2O(g)

What are the respective coefficients when the equation is balanced with the smallest whole numbers?
a.	1, 1, 1, 1	
b.	1, 2, 1, 2	
c.	2, 2, 2, 4	
d.	2, 3, 2, 4	
e.	2, 4, 6, 4	

____	2.	Aluminum reacts with oxygen to produce aluminum oxide.

4 Al(s) + 3 O2(g) ® 2 Al2O3(s)

If 10.0 moles of Al react with excess O2, how many moles of Al2O3 can be formed?
a.	1.0 mol	
b.	2.0 mol	
c.	2.5 mol	
d.	5.0 mol	
e.	10.0 mol	

____	3.	The complete combustion of 0.40 moles of butane gas, C4H10, will
a.	consume 0.40 mol O2 and produce 0.20 mol CO2.	
b.	consume 0.80 mol O2 and produce 0.40 mol CO2.	
c.	consume 1.3 mol O2 and produce 0.80 mol CO2.	
d.	consume 2.6 mol O2 and produce 1.6 mol CO2.	
e.	consume 5.2 mol O2 and produce 3.2 mol CO2.	

____	4.	If 46.1 g Zn at 18.0 °C is placed in 80.0 g H2O at 75.0 °C, what is the final temperature of the mixture? The specific heat capacities of zinc and water are 0.388 J/g·K and 4.184 J/g·K, respectively.
a.	20.9 °C	
b.	27.3 °C	
c.	64.5 °C	
d.	65.7 °C	
e.	72.1 °C	

____	5.	What is a correct method for determining how many moles of calcium oxide are produced in the reaction of 10.0 g calcium with excess oxygen?

2 Ca(s) + O2(g) ® 2 CaO(s)

a.	10.0 g Ca =	
b.	10.0 g Ca =	
c.	10.0 g Ca =	
d.	10.0 g Ca =	
e.	10.0 g Ca =	

____	6.	Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol).

C7H6O3(s) + C4H6O3(l) ® C9H8O4(s) + C2H4O2(l)

If 2.04 g of C9H8O4 (M = 180.2 g/mol) is produced from the reaction of 3.00 g C7H6O3 and 5.40 g C4H6O3, what is the percent yield?
a.	14.2%	
b.	21.4%	
c.	24.3%	
d.	52.1%	
e.	68.0%	

____	7.	Which of the following statements are correct?

1.	Salts of phosphate ion are insoluble in water, with the exception of those with NH4+ and alkali metal cations.	
2.	All salts of nitrate ion are soluble in water.	
3.	Most salts of ammonium ion are soluble in water.	

a.	1 only	
b.	2 only	
c.	3 only	
d.	1 and 2	
e.	1, 2, and 3	

____	8.	A precipitate will form when aqueous Hg(NO3)2 is added to an aqueous solution of ____.
a.	KNO3	
b.	Cu(NO3)2	
c.	KI	
d.	Ca(ClO4)2	
e.	NaNO3	

____	9.	What is the net ionic equation for the reaction of aqueous sodium carbonate with aqueous iron(III) chloride?
a.	3 Na+(aq) + Fe3+(aq) ® Na3Fe(s)	
b.	Na+(aq) + Cl-(aq) ® NaCl(s)	
c.	3 Na2CO3(aq) + 2 FeCl3(aq) ® 6 NaCl(aq) + Fe2(CO3)3(aq)	
d.	2 Fe3+(aq) + 3 CO32-(aq) ® Fe2(CO3)3(s)	
e.	CO32-(aq) + Cl-(aq) ® CO2(g) + Cl2O(s)	

____	10.	What is the net ionic equation for the reaction of aqueous lithium hydroxide and aqueous nitric acid?
a.	H+(aq) + LiOH(aq) ® H2O(l) + Li+(aq)	
b.	H+(aq) + OH-(aq) ® H2O(l)	
c.	HNO3(aq) + LiOH(aq) ® H2O(l) + LiNO3(aq)	
d.	Li+(aq) + NO3-(aq) ® LiNO3(aq)	
e.	LiOH(aq) + H2O(l) ® H+(aq) + Li(OH)2(s)	

____	11.	What are the spectator ions in the reaction between aqueous perchloric acid and aqueous potassium hydroxide?
a.	H+, ClO4-, K+, and OH-	
b.	H+ and OH-	
c.	K+ and ClO4-	
d.	H+ and ClO4-	
e.	K+ and OH-	

____	12.	Which species in the reaction below undergoes oxidation?

Sn(s) + 2 H+(aq) ®  Sn2+(aq) + H2(g)

a.	Sn	
b.	H+	
c.	Sn2+	
d.	H2	
e.	No compound is oxidized.	

____	13.	What is the oxidation number of each atom in potassium nitrate, KNO3?
a.	K = +1, N = -3, O = -2	
b.	K = +1, N = +5, O = -2	
c.	K = +1, N = -3, O = +2	
d.	K = -1, N = +3, O = -2	
e.	K = 0, N = 0, O = 0	

____	14.	Which of the following types of energy is a form of potential energy?
a.	sound energy	
b.	electrical energy	
c.	thermal energy	
d.	gravitational energy	
e.	mechanical energy	

____	15.	Specific heat capacity is
a.	the quantity of heat needed to change 1.00 g of a substance by 1.00 K.	
b.	the mass of a substance that 1.00 J of energy will heat by 1.00 K.	
c.	the mass of a substance that 1.00 cal of energy will heat by 1.00 K.	
d.	the temperature change undergone when 1.00 g of a substance absorbs 4.184 J.	
e.	the quantity of heat required to melt 4.184 g of a substance.	

____	16.	Which one of the following statements is INCORRECT?
a.	In an exothermic process heat is transferred from the system to the surroundings.	
b.	The greater the heat capacity of an object, the more thermal energy it can store.	
c.	The SI unit of specific heat capacity is joules per gram per Kelvin.	
d.	The specific heat capacity has a positive value for liquids and a negative value for gases.	
e.	When heat is transferred from the system to the surroundings, q is negative.	

____	17.	If 136 J is required to change the temperature of 8.75 g of nickel by 35.0 K, what is the specific heat capacity of mercury?
a.	0.0294 J/g·K	
b.	0.311 J/g·K	
c.	0.417 J/g·K	
d.	0.444 J/g·K	
e.	2.25 J/g·K	

____	18.	If the same amount of heat is added to 1.30 g samples of each of the metals below, which metal will experience the smallest temperature change?

Metal	Specific Heat Capacity (J/g·K)	
Al	0.897	
Au	0.129	
Cu	0.385	
Fe	0.449	
K	0.753	

a.	K	
b.	Au	
c.	Cu	
d.	Fe	
e.	Al	

MC_Chem1A_Sp08_LabQuiz2
Answer Section

MULTIPLE CHOICE

	1.	ANS:	D	PTS:	1	OBJ:	4.2 Balancing Chemical Equations

	2.	ANS:	D	PTS:	1	
OBJ:	4.3 Mass Relationships in Chemical Reactions: Stoichiometry	

	3.	ANS:	D	PTS:	1	
OBJ:	4.3 Mass Relationships in Chemical Reactions: Stoichiometry	

	4.	ANS:	E	PTS:	1	OBJ:	6.2 Specific Heat Capacity and Heat Transfer

	5.	ANS:	E	PTS:	1	
OBJ:	4.3 Mass Relationships in Chemical Reactions: Stoichiometry	

	6.	ANS:	D	PTS:	1	OBJ:	4.5 Percent Yield	

	7.	ANS:	E	PTS:	1	OBJ:	5.1 Properties of Compounds in Aqueous Solution

	8.	ANS:	C	PTS:	1	OBJ:	5.2 Precipitation Reactions

	9.	ANS:	D	PTS:	1	OBJ:	5.2 Precipitation Reactions

	10.	ANS:	B	PTS:	1	OBJ:	5.4 Reactions of Acids and Bases

	11.	ANS:	C	PTS:	1	OBJ:	5.4 Reactions of Acids and Bases

	12.	ANS:	A	PTS:	1	OBJ:	5.7 Oxidation-Reduction Reactions

	13.	ANS:	B	PTS:	1	OBJ:	5.7 Oxidation-Reduction Reactions

	14.	ANS:	D	PTS:	1	OBJ:	6.1 Energy: Some Basic Principles

	15.	ANS:	A	PTS:	1	OBJ:	6.2 Specific Heat Capacity and Heat Transfer

	16.	ANS:	D	PTS:	1	OBJ:	6.2 Specific Heat Capacity and Heat Transfer

	17.	ANS:	D	PTS:	1	OBJ:	6.2 Specific Heat Capacity and Heat Transfer

	18.	ANS:	E	PTS:	1	OBJ:	6.2 Specific Heat Capacity and Heat Transfer