CHM-201 General Chemistry and Laboratory I
Unit #2 – Take Home Test – Due March 9, 2017
Directions: Complete this test and pass in the answer sheet (also posted) on or before the due date. Please pass in only the
answer sheet. On the answer sheet, be sure to enter your ZipID (the last five digits of your student ID) and fill in the
appropriate bubbles. Record your answers unambiguously – ambiguous answers are wrong. Do not cross out answers – either
erase/cover them completely or print a new answer sheet. There is no need to fill in the version of the test. Absolutely no
papers will be accepted after the due date.
1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison
of the relative numbers of bromine and neon atoms in 1,000 g of each element?
A) The number of bromine and neon atoms is the same.
B) There are one thousand times as many bromine atoms as neon atoms.
C) There are one thousand times as many neon atoms as bromine atoms.
D) There are four times as many neon atoms as bromine atoms.
E) There are four times as many bromine atoms as neon atoms.
2. Calculate the average atomic mass of element X using the following data:
Isotope
28X
Abundance
Mass
92.223%
27.9769amu
29X
4.685%
28.9764amu
30X
3.092%
29.9737amu
A) 25.7947 amu
B) 28.0855 amu
C) 28.09 amu
D) 27.99 amu
E) 28.0858 amu
3. One mole of iron
A) is heavier than one mole of lead (Pb).
B) is 77.0 g of iron.
C) is 26.0 g of iron.
D) weighs the same as one mole of lead.
E) None of the above.
4. Calculate the number of moles of H2O in 50.0 g of water.
A) 2.77 mol
B) 0.360 mol
C) 9.00 mol
D) 18.0 mol
E) 0.0550 mol
5. Calculate the molar mass of Ba(NO3)2.
A) 199.3 g/mol
B) 323.3 g/mol
C) 247.3 g/mol
D) 261.3 g/mol
E) 398.6 g/mol
6. Calculate the mass of 4.50 moles of Ca3PO4.
A) 215 g
B) 968 g
C) 0.0209 g
D) 87.1 g
E) 392 g
7. How many moles of C are in 1.22 moles of C6H12O6?
A) 7.32 moles C
B) 87.9 moles C
C) 1.22 moles C
D) 14.7 moles C
E) 2.44 moles C
8. How many moles of O are there in 65.2 g C2H5OH?
A) 1.41 mol
B) 7.08 mol
C) 8.49 mol
D) 4.08 mol
E) 6.00 mol
9. Calculate the mass of N in 2.34 g of N2H4?
A) 4.68 g N
B) 65.6 g N
C) 28.02 g N
D) 2.05 g N
E) 2.34 g N
10. What is the mass of 0.0825 moles of UF6?
A) 352 g
B) 29.0 g
C) 1.37 × 10–4 g
D) 2.90 g
E) 8.25 g
11. The mineral manganosite is a compound of 55Mn and 16O. If 77% of the mass of manganosite is due to manganese, what is the
empirical formula of manganosite?
A) MnO
B) Mn2O
C) Mn2O2
D) MnO2
E) none of these
12. An unknown compound with a molar mass of 155.06 g/mol consists of 46.47% C, 7.80% H, and 45.72% Cl. Find the molecular
formula for the compound.
A) CHCl
B) C9H18Cl3
C) C6H12Cl
D) C6H12Cl2
E) C3H6Cl
13. What is the coefficient of H2O when the equation below is properly balanced?
___ PCl3(l) + ___ H2O(l) → ___ H3PO3(aq) + ___ HCl(aq)
A) 1
B) 2
C) 3
D) 5
E) none of these
14. Ammonia reacts with oxygen to form nitric oxide and water vapor:
4NH3 + 5O2 → 4NO + 6H2O
When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent?
A) NH3
B) O2
C) NO
D) H2O
E) No reagent is limiting.
15. Chlorine gas reacts with phosphorus to produce phosphorus pentachloride. How many grams of PCl 5 are produced from 3.5 g of
Cl2 and excess P?
5Cl2(g) + 2P(s) → 2PCl5(s)
A) 1.4 g
B) 4.1 g
C) 8.2 g
D) 0.020 g
E) 730 g
16. Hydrogen chloride gas can be prepared by the following reaction:
2NaCl(s) + H2SO4(aq) → 2HCl(g) + Na2SO4(s)
How many grams of HCl can be prepared from 2.00 mol H 2SO4 and 2.56 mol NaCl?
A) 7.30 g
B) 93.3 g
C) 146 g
D) 150 g
E) 196 g
17. One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na3(CO3)(HCO3)×2H2O, as
shown in the following reaction:
2Na3(CO3)(HCO3)×2H2O(s) → 3Na2CO3(s) + CO2(g) + 5H2O(g)
When 15 metric tons (1 × 103 kg) of trona is decomposed, 11 metric tons of Na 2CO3 is recovered. What is the percent yield of this
reaction? (1 metric ton = 103 kg) (Hint: Work this problem as though the masses were expressed in grams instead of kilograms. The
units will cancel anyway.)
A) 13%
B) 42%
C) 65%
D) 73%
E) 95%
18. Identify the major ionic species present in an aqueous solution of C6H12O6 (glucose).
A) 6 C-, 12 H+, 6 OB) 6 C+, 12 H+, 6 O2C) 6 CH2+, 6 O2D) C6+, 12 H+, 6 O2E) no ions are present
19. Based on the solubility rules, which of the following compounds should be insoluble in water?
A) CaCO3
B) (NH4)2CO3
C) Na2CO3
D) K2CO3
E) KNO3
20. Which of the following will occur when solutions of CuSO 4(aq) and BaCl2(aq) are mixed?
A) A precipitate of CuCl2 will form; Ba2+ and SO42– are spectator ions.
B) A precipitate of CuSO4 will form; Ba2+ and Cl– are spectator ions.
C) A precipitate of BaSO4 will form; Cu2+ and Cl– are spectator ions.
D) A precipitate of BaCl2 will form; Cu2+ and SO42– are spectator ions.
E) No precipitate will form.
21. Identify the correct net ionic equation for the reaction that occurs when solutions of AgNO3 and NH4Cl are mixed.
A) AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4Cl(aq)
B) NH4+(aq) + NO3-(aq) → NH4NO3(s)
C) AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4Cl(s)
D) Ag+(aq) + Cl-(aq) → AgCl(s)
E) AgNO3(aq) + NH4+(aq) → NH4AgNO3(s)
22. For which one of the following acids is chlorine in the +5 oxidation state?
A) HCl
B) HClO
C) HClO2
D) HClO3
E) HClO4
23. Which one of the following is a redox reaction?
A) 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
B) 2KBr(aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbBr2(s)
C) CaBr2(aq) + H2SO4(aq) → CaSO4(s) + 2HBr(g)
D) H+(aq) + OH– (aq) → H2O(l)
E) CO32– (aq) + HSO4–(aq) → HCO3– (aq) + SO42– (aq)
24. Identify the reducing agent in the following chemical reaction.
5Fe2+(aq) + MnO4–(aq)+ 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
A) Fe2+
B) MnO4–
C) H+
D) Mn2+
E) Fe3+
25. What mass of C6H12O6 (glucose) is needed to prepare 0.450 L of a 0.650 M solution of glucose in water?
A) 0.293 g
B) 293 g
C) 0.692 g
D) 52.7 g
E) 125 g
26. A 3.682 g sample of KClO 3 is dissolved in enough water to give 375 mL of solution. What is the chlorate ion concentration in this
solution?
A) 3.00 × 10–2 M
B) 4.41 × 10–2 M
C) 0.118 M
D) 1.65 × 10–2 M
E) 8.01 × 10–2 M
27. What volume of concentrated sulfuric acid (18.4 M) is required to make 100.0 mL of a 2.5 M nitric acid solution?
A) 13.5 mL
B) 27 mL
C) 14 mL
D) 6.75 mL
E) None of the above
28. During a titration the following data were collected. A 10.0 mL portion of an unknown monoprotic acid solution was titrated with
1.0 M NaOH; 40.0 mL of the base were required to neutralize the sample. How many moles of acid are present in 2.0 liters of this
unknown solution?
A) 6.0 moles
B) 7.0 moles
C) 8.0 moles
D) 9.0 moles
E) None of the above