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- Calcium fluoride, CaF 2 , is a source of fluorine and is used to fluoridate drinking water. Calculate its formula mass. A. 118.15 g/mol B. 99.15 g/mol C. 78.07 g/mol D. 59.08 g/mol E. 50.01 g/mol
- Calculate the molecular mass of tetraphosphorus decaoxide, P 4 O 10 , a corrosive substance which can be used as a drying agent. A. 469.73 g/mol B. 283.89 g/mol C. 190.97 g/mol D. 139.88 g/mol E. 94.97 g/mol
- Calculate the molecular or formula mass of rubidium carbonate, Rb 2 CO 3. A. 340.43 g/mol B. 255.00 g/mol C. 230.94 g/mol D. 145.47 g/mol E. 113.48 g/mol
- Calculate the molecular or formula mass of (NH 4 ) 3 AsO 4. A. 417.80 g/mol B. 193.03 g/mol C. 165.02 g/mol D. 156.96 g/mol E. 108.96 g/mol
- Aluminum sulfate, Al 2 (SO 4 ) 3 , is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molecular or formula mass. A. 450.06 g/mol B. 342.15 g/mol C. 315.15 g/mol D. 278.02 g/mol E. 74.98 g/mol
- Calculate the molar mass of Ca(BO 2 ) 2 ·6H 2 O. A. 273.87 g/mol B. 233.79 g/mol C. 183.79 g/mol D. 174.89 g/mol E. 143.71 g/mol
- Calculate the molecular mass of potassium permanganate, KMnO 4. A. 52 g/mol B. 70 g/mol C. 110 g/mol D. 158 g/mol E. 176 g/mol
- Calculate the molecular mass of menthol, C 10 H 20 O. A. 156 g/mol B. 140 g/mol C. 29 g/mol D. 146 g/mol E. 136 g/mol
- What is the molecular mass of acetaminophen, C 8 H 9 NO 2? A. 43 g/mol B. 76 g/mol C. 151 g/mol D. 162 g/mol E. 125 g/mol
- What is the molar mass of nicotine, C 10 H 14 N 2? A. 134 g/mol B. 148 g/mol C. 158 g/mol D. 210 g/mol E. 162 g/mol
- Household sugar, sucrose, has the molecular formula C 12 H 22 O 11. What is the % of carbon in sucrose, by mass? A. 26.7% B. 33.3% C. 41.4% D. 42.1% E. 52.8%
- What is the percent carbon in CH 3 CH 2 OH? A. 13% B. 24% C. 35% D. 46% E. 52%
- What is the percent sodium in sodium carbonate? A. 43.4% B. 11.3% C. 45.3% D. 27.7% E. 23%
- What is the percent sulfur in iron (III) sulfate? A. 28% B. 32% C. 24% D. 48% E. 42%
- What is the coefficient of H 2 O when the following equation is properly balanced with the smallest set of whole numbers? Na + H 2 O → NaOH + H 2 A. 1 B. 2 C. 3 D. 4 E. 5
- What is the coefficient of H 2 O when the following equation is properly balanced with smallest set of whole numbers? Al 4 C 3 + H 2 O → Al(OH) 3 + CH 4 A. 3 B. 4 C. 6 D. 12 E. 24
- When balanced with smallest set of whole numbers, the coefficient of O 2 in the following equation is:
C 2 H 4 + O 2 → CO 2 + H 2 O A. 1 B. 2 C. 3 D. 4 E. 6
- When a chemical equation is balanced, it will have a set of whole number coefficients that cannot be reduced to smaller whole numbers. What is the coefficient for O 2 when the following combustion reaction of a hydrocarbon is balanced? C 7 H 14 + O 2 → CO 2 + H 2 O A. 42 B. 21 C. 11 D. 10 E. None of the answers is correct.
- What is the coefficient preceding O 2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? C 18 H 36 O 2 + O 2 → CO 2 + H 2 O A. 1 B. 8 C. 9 D. 26 E. 27
- What is the coefficient of H 2 SO 4 when the following equation is properly balanced with the smallest set of whole numbers? Ca 3 (PO 4 ) 2 + H 2 SO 4 → CaSO 4 + H 3 PO 4 A. 3 B. 8 C. 10 D. 11
E. None of the answers is correct.
- What is the average mass, in grams, of one atom of iron (NA = 6.022 × 10^23 mol-1)? A. 6.02 × 10^23 g B. 1.66 × 10-24^ g C. 9.28 × 10-23^ g D. 55.85 g E. 55.85 × 10-23^ g
- What is the mass, in grams, of one arsenic atom (NA = 6.022 × 10^23 mol-1)? A. 5.48 × 10-23^ g B. 33.0 g C. 74.9 g D. 1.24 × 10-22^ g E. 8.04 × 10^21 g
- What is the mass of one copper atom (NA = 6.022 × 10^23 mol-1)? A. 1.055 × 10-22^ g B. 63.55 g C. 1 amu D. 1.66 × 10-24^ g E. 9.476 × 10^21 g
- The mass of 1.21 × 10^20 atoms of sulfur (NA = 6.022 × 10^23 mol-1) is: A. 3.88 × 10^21 g B. 2.00 mg C. 32.06 g D. 6.44 mg E. 2.00 × 10-4^ g
- The mass of 1.63 × 10^21 silicon atoms (NA = 6.022 × 10^23 mol-1) is: A. 2.71 × 10-23^ g B. 4.58 × 10^22 g C. 28.08 g D. 1.04 × 10^4 g E. 7.60 × 10-2^ g
- Determine the number of ammonia molecules in 4.85 g of ammonia (NA = 6.022 × 10^23 mol-1). A. 2.92 x 10^23 B. 4.73 x 10- C. 1.24 x 10^23 D. 5.83 x 10- E. 1.71 x 10^23
- What is the mass of 7.80 × 10^18 carbon atoms (NA = 6.022 × 10^23 mol-1)? A. 1.30 × 10 -5^ g B. 6.43 × 10^3 g C. 7.80 × 10^18 g D. 1.56 × 10 -4^ g E. 12.01 g
- What is the mass in grams of 0.250 mol of the common antacid calcium carbonate? A. 4.00 × 10^2 g B. 25.0 g C. 17.0 g D. 4.00 × 10-2^ g E. 2.50 × 10-3^ g
- Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH) 2. A. 3.28 mol B. 2.32 mol C. 0.431 mol D. 0.305 mol E. 0.200 mol
- Phosphorus pentachloride, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of phosphorus pentachloride. A. 5.38 mol B. 3.55 mol C. 0.583 mol D. 0.282 mol E. 0.186 mol
- Aluminum oxide, Al 2 O 3 , is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al 2 O 3. A. 2.377 mol B. 2.146 mol C. 1.105 mol D. 0.4660 mol E. 0.4207 mol
- Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 × 10^20 molecules of sulfur trioxide. A. 6.06 × 10-4^ g B. 2.91 × 10-2^ g C. 4.85 × 10-2^ g D. 20.6 g E. 1650 g
- Calculate the mass in grams of 8.35 × 10^22 molecules of CBr 4. A. 0.0217 g B. 0.139 g C. 7.21 g D. 12.7 g E. 46.0 g
- The number of hydrogen atoms in 0.050 mol of C 3 H 8 O 3 is: A. 3.0 × 10^22 H atoms B. 1.2 × 10^23 H atoms C. 2.4 × 10^23 H atoms D. 4.8 × 10^23 H atoms E. None of the answers is correct.
- What is the mass of 0.0250 mol of P 2 O 5? A. 35.5 g B. 5676 g C. 0.0250 g D. 1.51 × 10^22 g E. 3.55 g
- Calculate the mass of 3.00 moles of CF 2 Cl 2. A. 3.00 g B. 174 g
- Gadolinium oxide, a colorless powder which absorbs carbon dioxide from the air, contains 86.76 mass % Gd. Determine its empirical formula. A. Gd 2 O 3 B. Gd 3 O 2 C. Gd 3 O 4 D. Gd 4 O 3 E. GdO
- Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. Determine its empirical formula. A. HNO B. H 2 NO 2 C. HN 6 O 16 D. HN 16 O 7 E. H 2 NO 3
- Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula? A. NH 2 O 5 B. N 2 H 4 O 4 C. N 3 H 3 O 3 D. N 4 H 8 O 2 E. N 2 H 2 O 4
- A compound of bromine and fluorine is used to make UF 6 , which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula. A. BrF B. BrF 2 C. Br 2 F 3 D. Br 3 F E. BrF 3
- A compound containing chromium and silicon contains 73.52 mass percent chromium. Determine its empirical formula. A. CrSi 3 B. Cr 2 Si 3 C. Cr 3 Si D. Cr 3 Si 2 E. Cr 2 S
- The empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine is: A. U 2 F B. U 3 F 4 C. UF 4 D. UF 6 E. UF 8
- The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O The molar mass of this compound is 284.5 g/mol. What is the molecular formula of the compound? A. C 10 H 6 O B. C 9 H 18 O C. C 16 H 28 O 4
- D. C 20 H 12 O
- E. C 18 H 36 O
B. 0.629 g C. 13.04 g D. 17.63 g E. 6.52 g
- How many grams of nitrogen are required to react with 2.79 g of hydrogen to produce ammonia? A. 25.8 g B. 13.0 g C. 78.2 g D. 38.7 g E. 77.4 g
- How many grams of nitrogen are required to react with hydrogen to produce 13.6 g of ammonia? A. 11.2 g B. 0.06 g C. 22.4 g D. 16.5 g E. 44.8 g
- What mass, in grams, of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water? A. 28.1 g B. 14.04 g C. 4.96 g D. 7.02 g E. 400.0 g
- How many grams of lead (II) chloride are produced when 13.87 g lead (II) nitrate combines with hydrochloric acid to produce lead (II) chloride and nitric acid? A. 5.82 g B. 1.19 g C. 0.086 g D. 11.65 g E. 16.52 g
- How many grams of calcium are required to react with 7.75 g of water to produce calcium hydroxide and hydrogen gas? A. 8.62 g B. 34.5 g C. 4.31 g D. 3.48 g E. 17.2 g
- How many grams of oxygen are required to react with calcium to produce 44.8 g calcium oxide? A. 12.8 g B. 25.6 g C. 6.4 g D. 0.05 g E. 51.1 g
- How many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides) are needed to form 485 g of sulfur tetrafluoride?
3SCl 2 (l) + 4NaF(s) → SF 4 (g) + S 2 Cl 2 (l) + 4NaCl(s) A. 1940 g B. 1510 g C. 754 g D. 205 g E. 51.3 g
- Hydrochloric acid can be prepared by the following reaction:
2NaCl(s) + H 2 SO 4 (aq) → 2HCl(g) + Na 2 SO 4 (s)
How many grams of HCl can be prepared from 2.00 mol H 2 SO 4 and 150 g NaCl? A. 7.30 g B. 93.5 g C. 146 g D. 150 g E. 196 g
- Calculate the mass of FeS formed when 9.42 g of Fe reacts with 8.50 g of S.
Fe(s) + S(s) → FeS(s) A. 17.9 g B. 87.9 g C. 26.0 g D. 14.8 g E. 1.91 × 10-3^ g
- What is the limiting reactant when 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia and how many grams of ammonia are produced? A. Hydrogen is the limiting reactant and 0.22 g of ammonia are produced. B. Nitrogen is the limiting reactant and 2.07 g of ammonia are produced. C. Nitrogen is the limiting reactant and 4.15 g of ammonia are produced. D. Hydrogen is the limiting reactant and 23.5 g of ammonia are produced. E. Hydrogen is the limiting reactant and 15.8 g of ammonia are produced.
- What is the limiting reactant when 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide and how many grams of calcium oxide are produced? A. Calcium is the limiting reactant and 47.1 g of calcium oxide are produced. B. Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced. C. Calcium is the limiting reactant and 47.1 g of calcium dioxide are produced. D. Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced. E. Calcium is the limiting reactant and 23.6 g of calcium oxide are produced.
- What is the limiting reactant when 31.3 g of manganese (II) chloride, 48.3 g of chlorine, and 25.7 g of water react to produce manganese (IV) oxide and how much hydrochloric acid is produced? A. Manganese (II) chloride is the limiting reactant and 8.40 g of hydrochloric acid is produced. B. Chlorine is the limiting reactant and 6.21 g of hydrochloric acid is produced. C. Chlorine is the limiting reactant and 24.8 g of hydrochloric acid is produced. D. Manganese (II) chloride is the limiting reactant and 36.3 g of hydrochloric acid is produced. E. Water is the limiting reactant and 52 g of hydrochloric acid is produced.
- Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for organic reactions. A mixture of 82.49 g of aluminum and 117.65 g of oxygen is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. A. Oxygen is the limiting reactant; 19.81 g of aluminum remain. B. Oxygen is the limiting reactant; 35.16 g of aluminum remain. C. Aluminum is the limiting reactant; 16.70 g of oxygen remain. D. Aluminum is the limiting reactant; 35.16 g of oxygen remain. E. Aluminum is the limiting reactant; 44.24 g of oxygen remain.
- Magnesium (used in the manufacture of light alloys) reacts with iron (III) chloride to form magnesium chloride and iron. A mixture of 41.0 g of magnesium and 175 g of iron (III) chloride is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete. A. Limiting reactant is Mg; 67 g of FeCl 3 remain. B. Limiting reactant is Mg; 134 g of FeCl 3 remain. C. Limiting reactant is Mg; 104 g of FeCl 3 remain. D. Limiting reactant is FeCl 3 ; 2 g of Mg remain. E. Limiting reactant is FeCl 3 ; 87 g of Mg remain.
- Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride. A. Potassium is the limiting reactant; 2.47 g of chlorine remain. B. Potassium is the limiting reactant; 7.23 g of chlorine remain. C. Chlorine is the limiting reactant; 4.64 g of potassium remain. D. Chlorine is the limiting reactant; 2.70 g of potassium remain. E. No limiting reagent: the reactants are present in the correct stoichiometric ratio.
- Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75. g of phosphorus and 38.7 g of oxygen produce 43.3 g of P 4 O 6 , what is the percent yield for the reaction?
A. 57.5% B. 48.8% C. 38.0% D. 32.4% E. 16.3%
- What is the percent yield for the reaction
PCl 3 (g) + Cl 2 (g) → PCl 5 (g)
if 119.3 g of PCl 5 are formed when 61.3 g of Cl 2 react with excess PCl 3? A. 195% B. 85.0% C. 66.3% D. 51.4% E. 43.7%
- Methanol (CH 4 O) is converted to bromomethane (CH 3 Br) as follows:
CH 4 O + HBr → CH 3 Br + H 2 O
If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield? A. 40.9% B. 82.6% C. 100.% D. 121% E. 245%
E. 108 g
- Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor:
4NH 3 + 5O 2 → 4NO + 6H 2 O What is the theoretical yield of water, in moles, when 40.0 g NH 3 and 50.0 g O 2 are mixed and allowed to react? A. 1.30 mol B. 1.57 mol C. 1.87 mol D. 3.53 mol E. 2.87 mol
- What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 mole of V 2 O 5 with 6.0 mole of calcium based on the following chemical equation? V 2 O 5 (s) + 5Ca(l) → 2V(l) + 5CaO(s) A. 1.0 mol B. 1.6 mol C. 2.0 mol D. 2.4 mol E. 4.0 mol
- What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V 2 O 5 with 4.0 mole of calcium based on the following chemical equation? V 2 O 5 (s) + 5Ca(l) → 2V(l) + 5CaO(s) A. 1.0 mol B. 1.6 mol C. 2.0 mol D. 0.80 mol E. 3.2 mol
- What is the theoretical yield of vanadium that can be produced by the reaction of 40.0g of V 2 O 5 with 40.0g of calcium based on the following chemical equation? V 2 O 5 (s) + 5Ca(l) → 2V(l) + 5CaO(s) A. 11.2 g B. 5.6 g C. 22.4 g D. 40.0 g E. 20.3 g
- How many grams of Cr can be produced by the reaction of 44.1 g of Cr 2 O 3 with 35.0 g of Al according to the following chemical equation? 2Al + Cr 2 O 3 → Al 2 O 3 + 2Cr A. 7.56 g B. 30.2 g C. 67.4 g D. 104 g E. 60.4 g
- What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al 2 O 3 + 3C → 2Al + 3CO A. 30.0 g B. 7.9 g C. 101.2 g
