Exam-Practice for ACS
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) How many significant figures are there in the answer to the following problem? 1)
(9.992 × 3.200) + 0.610 = ?
A) one B) two C) three D) four
2) A student performs an experiment to determine the density of a sugar solution. She obtains the 2)
following results: 1.71 g/mL, 1.73 g/mL, 1.67 g/mL, 1.69 g/mL. If the actual value for the density of
the sugar solution is 1.40 g/mL, which statement below best describes her results?
A) Her results are precise, but not accurate.
B) Her results are neither precise nor accurate.
C) Her results are both precise and accurate
D) Her results are accurate, but not precise.
E) It isn't possible to determine with the information given.
3) Choose the homogeneous mixture from the list below. 3)
A) salad dressing
B) cola
C) mud
D) salsa
E) ice water
4) A piece of metal ore weighs 8.25 g. When a student places it into a graduated cylinder containing 4)
water, the liquid level rises from 21.25 mL to 26.47 mL. What is the density of the ore?
A) 0.312 g/mL B) 3.21 g/mL C) 1.58 g/mL D) 0.633 g/mL
5) Determine the number of protons, neutrons and electrons in the following: 5)
40
X
18
A) p+ = 18 n° = 18 e- = 22
B) p+ = 40 n° = 22 e- = 18
C) p+ = 22 n° = 18 e- = 18
D) p+ = 18 n° = 22 e- = 18
E) p+ = 18 n° = 22 e- = 40
6) Which of the following represent isotopes? 6)
32 32 31 34
A: X B: X C: X D: X
15 16 15 17
A) A and D B) A and B C) C and D D) A and C
7) In which of the following sets do all species have the same number of electrons? 7)
A) Ge, Se2- , Br- B) Br, Br-, Br+ C) F- , Ne, Mg2+ D) K+ , Rb+ , Cs+
1
, 8) Calculate the atomic mass of element "X", if it has 2 naturally occurring isotopes with the following 8)
masses and natural abundances:
X-45 44.8776 amu 32.88%
X-47 46.9443 amu 67.12%
A) 46.26 amu B) 45.91 amu C) 44.99 amu D) 46.84 amu E) 46.34 amu
9) Which of the following is an ionic compound? 9)
A) CH2O
B) SCl2
C) Cl2 O
D) PF5
E) Mg3(PO4 )2
10) Write the name for Sn(SO4 )2 . Remember that Sn forms several ions. 10)
A) tin sulfide
B) tin (I) sulfite
C) tin (I) sulfate
D) tin (IV) sulfate
E) tin (II) sulfite
11) Write the formula for barium nitrite. 11)
A) Ba(NO2 )2 B) B(NO2 )3 C) BaNO3 D) Ba3 N2 E) BN
12) Determine the name for N2 O5 . 12)
A) dinitrogen pentoxide
B) nitrogen tetroxide
C) nitrogen (II) oxide
D) nitrogen (IV) oxide
E) nitrogen oxide
13) Give the name for H2 SO4 . 13)
A) persulfuric acid
B) sulfurous acid
C) hyposulfurous acid
D) persulfurous acid
E) sulfuric acid
14) How many atoms of oxygen are contained in 47.6 g of Al2 (CO3 )3? The molar mass of Al2 (CO3 )3 is 14)
233.99 g/mol.
A) 1.23 × 1023 O atoms
B) 1.10 × 1024 O atoms
C) 3.68 × 1023 O atoms
D) 2.96 × 1024 O atoms
E) 2.87 × 1025 O atoms
2
, 15) Calculate the mass percent composition of sulfur in Al2 (SO4 )3 . 15)
A) 21.38 % B) 9.372 % C) 35.97 % D) 28.12 % E) 42.73 %
16) Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C 16)
and 34.73% O by mass.
A) C2 H6 O B) CHO C) C4 H13O2 D) CH3 O E) CH4 O3
17) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 17)
and 59.38 mg of H2 O. What is the empirical formula for the compound?
A) C6 HO3 B) C5 H2 O C) C3 H7 O D) C3 H6 O E) CHO
18) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous 18)
ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2 H3 O2 )2 (aq) + (NH4 )2 PO4 (aq) AlPO4 (s) + 2 NH 4 C2 H3 O2 (aq)
B) Al(C2 H3 O2 )2 (aq) + (NH3 )2 PO4 (aq) AlPO4 (s) + 2 NH 3 C2 H3 O2 (aq)
C) Al(CO2 )3 (aq) + (NH4 )3 PO3 (aq) AlPO3 (s) + 3 NH 4 CO2 (aq)
D) Al(CO3 )2 (aq) + (NH3 )2 PO4 (aq) AlPO4 (s) + 2 NH 3 CO3 (aq)
E) Al(C2 H3 O2 )3 (aq) + (NH4 )3 PO4 (aq) AlPO4 (s) + 3 NH4 C2 H3 O2 (aq)
19) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2 O3 react 19)
with excess Al according to the following reaction.
Fe2 O3 (s) + 2 Al(s) Al2 O3 (s) + 2 Fe(s)
A) 57.30 % B) 61.03 % C) 81.93 % D) 28.65 % E) 20.02 %
20) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8 H18 20)
with 4.000 moles of O2 .
2 C8 H18 + 25 O2 16 CO2 + 18 H2 O
A) 50.00% B) 25.00% C) 12.50% D) 20.00%
21) How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution? 21)
A) 58.40 g B) 14.60 g C) 43.83 g D) 175.3 g
22) What volume (in mL) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 22)
solution?
A) 69.4 mL B) 91.8 mL C) 10.9 mL D) 72.3 mL E) 14.4 mL
23) What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2 SO4 solution is required to 23)
neutralize a 25.0-mL sample of the NaOH solution?
A) 0.315 B) 0.400 C) 125 D) 0.801 E) 0.629
3
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) How many significant figures are there in the answer to the following problem? 1)
(9.992 × 3.200) + 0.610 = ?
A) one B) two C) three D) four
2) A student performs an experiment to determine the density of a sugar solution. She obtains the 2)
following results: 1.71 g/mL, 1.73 g/mL, 1.67 g/mL, 1.69 g/mL. If the actual value for the density of
the sugar solution is 1.40 g/mL, which statement below best describes her results?
A) Her results are precise, but not accurate.
B) Her results are neither precise nor accurate.
C) Her results are both precise and accurate
D) Her results are accurate, but not precise.
E) It isn't possible to determine with the information given.
3) Choose the homogeneous mixture from the list below. 3)
A) salad dressing
B) cola
C) mud
D) salsa
E) ice water
4) A piece of metal ore weighs 8.25 g. When a student places it into a graduated cylinder containing 4)
water, the liquid level rises from 21.25 mL to 26.47 mL. What is the density of the ore?
A) 0.312 g/mL B) 3.21 g/mL C) 1.58 g/mL D) 0.633 g/mL
5) Determine the number of protons, neutrons and electrons in the following: 5)
40
X
18
A) p+ = 18 n° = 18 e- = 22
B) p+ = 40 n° = 22 e- = 18
C) p+ = 22 n° = 18 e- = 18
D) p+ = 18 n° = 22 e- = 18
E) p+ = 18 n° = 22 e- = 40
6) Which of the following represent isotopes? 6)
32 32 31 34
A: X B: X C: X D: X
15 16 15 17
A) A and D B) A and B C) C and D D) A and C
7) In which of the following sets do all species have the same number of electrons? 7)
A) Ge, Se2- , Br- B) Br, Br-, Br+ C) F- , Ne, Mg2+ D) K+ , Rb+ , Cs+
1
, 8) Calculate the atomic mass of element "X", if it has 2 naturally occurring isotopes with the following 8)
masses and natural abundances:
X-45 44.8776 amu 32.88%
X-47 46.9443 amu 67.12%
A) 46.26 amu B) 45.91 amu C) 44.99 amu D) 46.84 amu E) 46.34 amu
9) Which of the following is an ionic compound? 9)
A) CH2O
B) SCl2
C) Cl2 O
D) PF5
E) Mg3(PO4 )2
10) Write the name for Sn(SO4 )2 . Remember that Sn forms several ions. 10)
A) tin sulfide
B) tin (I) sulfite
C) tin (I) sulfate
D) tin (IV) sulfate
E) tin (II) sulfite
11) Write the formula for barium nitrite. 11)
A) Ba(NO2 )2 B) B(NO2 )3 C) BaNO3 D) Ba3 N2 E) BN
12) Determine the name for N2 O5 . 12)
A) dinitrogen pentoxide
B) nitrogen tetroxide
C) nitrogen (II) oxide
D) nitrogen (IV) oxide
E) nitrogen oxide
13) Give the name for H2 SO4 . 13)
A) persulfuric acid
B) sulfurous acid
C) hyposulfurous acid
D) persulfurous acid
E) sulfuric acid
14) How many atoms of oxygen are contained in 47.6 g of Al2 (CO3 )3? The molar mass of Al2 (CO3 )3 is 14)
233.99 g/mol.
A) 1.23 × 1023 O atoms
B) 1.10 × 1024 O atoms
C) 3.68 × 1023 O atoms
D) 2.96 × 1024 O atoms
E) 2.87 × 1025 O atoms
2
, 15) Calculate the mass percent composition of sulfur in Al2 (SO4 )3 . 15)
A) 21.38 % B) 9.372 % C) 35.97 % D) 28.12 % E) 42.73 %
16) Determine the empirical formula for a compound that contains C, H and O. It contains 52.14% C 16)
and 34.73% O by mass.
A) C2 H6 O B) CHO C) C4 H13O2 D) CH3 O E) CH4 O3
17) Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 17)
and 59.38 mg of H2 O. What is the empirical formula for the compound?
A) C6 HO3 B) C5 H2 O C) C3 H7 O D) C3 H6 O E) CHO
18) Write a balanced equation to show the reaction of aqueous aluminum acetate with aqueous 18)
ammonium phosphate to form solid aluminum phosphate and aqueous ammonium acetate.
A) Al(C2 H3 O2 )2 (aq) + (NH4 )2 PO4 (aq) AlPO4 (s) + 2 NH 4 C2 H3 O2 (aq)
B) Al(C2 H3 O2 )2 (aq) + (NH3 )2 PO4 (aq) AlPO4 (s) + 2 NH 3 C2 H3 O2 (aq)
C) Al(CO2 )3 (aq) + (NH4 )3 PO3 (aq) AlPO3 (s) + 3 NH 4 CO2 (aq)
D) Al(CO3 )2 (aq) + (NH3 )2 PO4 (aq) AlPO4 (s) + 2 NH 3 CO3 (aq)
E) Al(C2 H3 O2 )3 (aq) + (NH4 )3 PO4 (aq) AlPO4 (s) + 3 NH4 C2 H3 O2 (aq)
19) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2 O3 react 19)
with excess Al according to the following reaction.
Fe2 O3 (s) + 2 Al(s) Al2 O3 (s) + 2 Fe(s)
A) 57.30 % B) 61.03 % C) 81.93 % D) 28.65 % E) 20.02 %
20) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8 H18 20)
with 4.000 moles of O2 .
2 C8 H18 + 25 O2 16 CO2 + 18 H2 O
A) 50.00% B) 25.00% C) 12.50% D) 20.00%
21) How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution? 21)
A) 58.40 g B) 14.60 g C) 43.83 g D) 175.3 g
22) What volume (in mL) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 22)
solution?
A) 69.4 mL B) 91.8 mL C) 10.9 mL D) 72.3 mL E) 14.4 mL
23) What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2 SO4 solution is required to 23)
neutralize a 25.0-mL sample of the NaOH solution?
A) 0.315 B) 0.400 C) 125 D) 0.801 E) 0.629
3
