MC_Chem1A_Fall07_LecExam2

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

____	1.	Calcium reacts with fluorine gas to produce calcium fluoride. How many moles of Ca will react with 1.0 moles of F2?
a.	0.50 mol	
b.	1.0 mol	
c.	1.5 mol	
d.	2.0 mol	
e.	4.0 mol	

____	2.	Copper reacts with nitric acid to produce copper(II) nitrate, nitrogen dioxide gas, and water.

Cu(s) + 4 HNO3(aq) ® Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O(l)

If you have 0.500 moles of Cu,
a.	you need at least 0.125 moles of HNO3 to produce 0.500 moles of Cu(NO3)2.	
b.	you need at least 0.250 moles of HNO3 to produce 0.500 moles of Cu(NO3)2.	
c.	you need at least 2.00 moles of HNO3 to produce 0.500 moles of Cu(NO3)2.	
d.	you need at least 2.00 moles of HNO3 to produce 1.00 moles of Cu(NO3)2.	
e.	you need at least 2.00 moles of HNO3 to produce 2.00 moles of Cu(NO3)2.	

____	3.	Sodium carbonate reacts with hydrochloric acid as shown below in an unbalanced chemical equation. What mass of CO2 is produced from the reaction of 2.94 g Na2CO3 with excess HCl?

Na2CO3(s) + HCl(aq) ® NaCl(aq) + CO2(g) + H2O(l)

a.	1.22 g	
b.	2.44 g	
c.	2.94 g	
d.	5.88 g	
e.	7.08 g	

____	4.	How many moles of potassium bromide can be produced from the reaction of 2.92 moles of potassium with 1.78 moles of bromine gas?

2 K(s) + Br2(g) ®  2 KBr(s)

a.	1.46 mol	
b.	1.78 mol	
c.	2.92 mol	
d.	3.56 mol	
e.	5.84 mol	

____	5.	The reaction of 10.0 g H2(g) with 10.0 g O2(g) yields 8.43 g H2O(g). What is the percent yield of this reaction?
a.	9.43%	
b.	27.3%	
c.	42.2%	
d.	66.8%	
e.	74.9%	

____	6.	Which one of the following compounds is a nonelectrolyte when dissolved in water?
a.	CH3CH2OH	
b.	ZnBr2	
c.	LiCl	
d.	Ca(NO3)2	
e.	KOH	

____	7.	If 0.10 mole of each of the following compounds is dissolved to a volume of 1.0 L in water, which one will have the highest concentration of dissolved ions?
a.	HF	
b.	NaOH	
c.	MgSO4	
d.	Al(NO3)3	
e.	CaI2	

____	8.	Which of the following compounds will be soluble in water: KNO3, Ca3(PO4)2, CuCl2, and Fe2S3?
a.	KNO3 and Ca3(PO4)2	
b.	KNO3 and CuCl2	
c.	Ca3(PO4)2 and Fe2S3	
d.	CuCl2 and Fe2S3	
e.	KNO3, Ca3(PO4)2, and Fe2S3	

____	9.	A white solid is either NaI or NaNO3. If an aqueous solution of the solid is prepared, the addition of which reagent will allow you to distinguish between the two compounds?
a.	NaOH	
b.	HCl	
c.	K3PO4	
d.	NH4Br	
e.	Pb(NO3)2	

____	10.	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)	

____	11.	Which of the following compounds is a weak base?
a.	LiOH	
b.	KCl	
c.	CH3CO2H	
d.	Sr(OH)2	
e.	NH3	

____	12.	Which of the following chemical equations is an acid-base reaction?
a.	2 HCl(aq) + Zn(s) ®  H2(g) + ZnCl2(aq)	
b.	HCl(aq) + NH3(aq) ®  NH4Cl(aq)	
c.	HCl(aq) + AgNO3(aq) ®  AgCl(s) + HNO3(aq)	
d.	Ba(OH)2(aq) + Na2SO4(aq) ®  BaSO4(s) + 2 NaOH(aq)	
e.	2 NaOH(aq) + CuCl2(aq) ®  Cu(OH)2(s) + 2 NaCl(aq)	

____	13.	Which compound is the oxidizing agent in the reaction below?

I-(aq) + ClO-(aq) ®  IO-(aq) + Cl-(aq)

a.	I-	
b.	H2O	
c.	Cl-	
d.	IO-	
e.	ClO-	

____	14.	What is the oxidation number of iodine in IO3-?
a.	-1	
b.	0	
c.	+3	
d.	+5	
e.	+7	

____	15.	Which of the following elements generally acts as a reducing agent?
a.	O2	
b.	H+	
c.	F-	
d.	F2	
e.	Na	

____	16.	If 2.891 g MgCl2 is dissolved in enough water to make 500.0 mL of solution, what is the molarity of the magnesium chloride solution?
a.	5.782 ´ 10-3 M	
b.	1.518 ´ 10-2 M	
c.	6.073 ´ 10-2 M	
d.	0.5505 M	
e.	5.782 M	

____	17.	A aqueous hydrochloric acid solution has a pH of 4.15. What mass of HCl is present in 1.0 L of this solution?
a.	7.2 ´ 10-5 g	
b.	2.6 ´ 10-3 g	
c.	0.58 g	
d.	23 g	
e.	150 g	

____	18.	Which one of the following statements is INCORRECT?
a.	Energy is neither created nor destroyed in chemical reactions.	
b.	Kinetic energy is the energy associated with motion.	
c.	Exothermic processes transfer heat from the surrounding into the system.	
d.	Increasing the thermal energy of a gas increases the motion of its atoms.	
e.	Energy is the capacity to do work.	

____	19.	If 50.0 g H2O at 13.6 °C is combined with 85.0 g H2O at 93.7 °C, what is the final temperature of the mixture? The specific heat capacity of water is 4.184 J/g·K.
a.	26.1 °C	
b.	40.0 °C	
c.	56.1 °C	
d.	64.0 °C	
e.	80.1 °C	

____	20.	The thermochemical equation for the combustion of butane is shown below.

C4H10(g) + 13/2 O2(g) ® 4 CO2(g) + 5 H2O(l) DH° = -2877 kJ

What is the enthalpy change for the following reaction?

16 CO2(g) + 20 H2O(l) ® 4 C4H10(g) + 26 O2(g)
a.	-5754 kJ	
b.	-719.2 kJ	
c.	+719.2 kJ	
d.	+5754 kJ	
e.	+1.151 ´ 104 kJ	

____	21.	Determine the heat of reaction for the oxidation of iron,

4 Fe(s) + 3 O2(g) ® 2 Fe2O3(s)

given the thermochemical equations below.

2 Fe(s) + 6 H2O(l) ® 2 Fe(OH)3(s) + 3 H2(g) DH = +321.8 kJ
2 H2O(l) ® 2 H2(g) + O2(g) DH = +571.7 kJ
Fe2O3(s) + 3 H2O(l) ® 2 Fe(OH)3(s) DH = +288.6 kJ

a.	-1648.7 kJ	
b.	-1182.1 kJ	
c.	-505.3 kJ	
d.	+360.5 kJ	
e.	+1447.1 kJ	

____	22.	Which of the following regions of the electromagnetic spectrum have longer wavelengths than visible light?

1.	FM radio waves	
2.	x-rays	
3.	microwaves	

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

____	23.	Which of the following regions of the electromagnetic spectrum has the lowest frequency?
a.	ultraviolet	
b.	infrared	
c.	visible	
d.	x-ray	
e.	gamma ray	

____	24.	A microwave oven emits radiation at a wavelength of 0.500 cm. What is the frequency of this radiation?
a.	1.67 ´ 10-11 s-1	
b.	6.67 ´ 10-7 s-1	
c.	2.00 s-1	
d.	1.50 ´ 106 s-1	
e.	6.00 ´ 1010 s-1	

____	25.	According to experiments concerned with the photoelectric effect, which of the following will increase the kinetic energy of an electron ejected from a metal surface?

1.	increasing the wavelength of the light striking the surface	
2.	increasing the frequency of the light striking the surface	
3.	increasing the number of photons of light striking the surface	

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

____	26.	A red laser pointer emits light at a wavelength of 635 nm. If the laser emits 7.5 ´ 10-4 J of energy per second in the form of visible radiation, how many photons per second are emitted from the laser?
a.	4.2 ´ 10-16 photons/sec	
b.	2.4 ´ 1015 photons/sec	
c.	6.3 ´ 1017 photons/sec	
d.	2.7 ´ 1022 photons/sec	
e.	1.8 ´ 1036 photons/sec	

____	27.	Which of the following transitions in a hydrogen atom would emit the lowest energy photon?
a.	n = 1 to n = 2	
b.	n = 3 to n = 2	
c.	n = 5 to n = 1	
d.	n = 2 to n = 8	
e.	n = 6 to n = 5	

____	28.	The Schrödinger wave equation
a.	calculates the position and momentum of an electron at any given time.	
b.	can be solved to determine the probability of finding an electron in a region of space.	
c.	proves that energy is equal to mass times the speed of light squared.	
d.	incorrectly predicts circular orbits of electrons around nuclei.	
e.	is used to calculate the velocity of an electron.	

____	29.	What type of orbital is designated n = 3, l = 2, ml = -1?
a.	3s	
b.	3p	
c.	3d	
d.	2f	
e.	2d	

____	30.	What shell contains a total of 9 orbitals?
a.	n = 1	
b.	n = 2	
c.	n = 3	
d.	n = 4	
e.	n = 5	

____	31.	Which of the following sets of quantum numbers refers to a 4p orbital?
a.	n = 1, l = 1, ml = -1	
b.	n = 1, l = 2, ml = -1	
c.	n = 4, l = 1, ml = 0	
d.	n = 4, l = 2, ml = -1	
e.	n = 4, l = 3, ml = +2	

____	32.	All of the following sets of quantum numbers are allowed EXCEPT
a.	n = 5, l = 3, ml = +2	
b.	n = 3, l = 2, ml = -1	
c.	n = 3, l = 0, ml = 0	
d.	n = 4, l = 4, ml = -2	
e.	n = 5, l = 3, ml = +3	

____	33.	Which of the following orbitals might have ml = -2?
a.	s	
b.	s and p	
c.	p and d	
d.	d and f	
e.	p, d, and f	

____	34.	The n = ____ shell is the lowest that may contain p-orbitals.
a.	2	
b.	3	
c.	4	
d.	5	
e.	6	

MC_Chem1A_Fall07_LecExam2
Answer Section

MULTIPLE CHOICE

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

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

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

	4.	ANS:	C	PTS:	1	
OBJ:	4.4 Reactions in which One Reactant is Present in Limited Supply	

	5.	ANS:	E	PTS:	1	
OBJ:	4.4 Reactions in which One Reactant is Present in Limited Supply	

	6.	ANS:	A	PTS:	1	OBJ:	5.1 Properties of Compounds in Aqueous Solution

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

	8.	ANS:	B	PTS:	1	OBJ:	5.1 Properties of Compounds in Aqueous Solution

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

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

	11.	ANS:	E	PTS:	1	OBJ:	5.3 Acids and Bases	

	12.	ANS:	B	PTS:	1	OBJ:	5.6 Classifying Reactions in Aqueous Solution

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

	14.	ANS:	D	PTS:	1	OBJ:	5.7 Oxidation-Reduction Reactions

	15.	ANS:	E	PTS:	1	OBJ:	5.7 Oxidation-Reduction Reactions

	16.	ANS:	C	PTS:	1	OBJ:	5.8 Measuring Concentrations of Compounds in Solution

	17.	ANS:	B	PTS:	1	OBJ:	5.9 pH | A Concentration Scale for Acids and Bases

	18.	ANS:	C	PTS:	1	OBJ:	6.1 Energy: Some Basic Principles

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

	20.	ANS:	E	PTS:	1	OBJ:	6.5 Enthalpy Changes for Chemical Reactions

	21.	ANS:	A	PTS:	1	OBJ:	6.7 Hess's Law	

	22.	ANS:	E	PTS:	1	OBJ:	7.1 Electromagnetic Radiation

	23.	ANS:	B	PTS:	1	OBJ:	7.1 Electromagnetic Radiation

	24.	ANS:	E	PTS:	1	OBJ:	7.1 Electromagnetic Radiation

	25.	ANS:	B	PTS:	1	OBJ:	7.2 Planck | Einstein | Energy | and Photons

	26.	ANS:	B	PTS:	1	OBJ:	7.2 Planck | Einstein | Energy | and Photons

	27.	ANS:	E	PTS:	1	OBJ:	7.3 Atomic Line Spectra and Niels Bohr

	28.	ANS:	B	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom

	29.	ANS:	C	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom

	30.	ANS:	C	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom

	31.	ANS:	C	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom

	32.	ANS:	D	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom

	33.	ANS:	D	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom

	34.	ANS:	A	PTS:	1	OBJ:	7.5 Quantum Mechanical View of the Atom