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Exam 3: Stoichiometry of Formulas and Equations

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Question 21

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Balance the following equation: UO₂(s) + HF(l) → UF₄(s) + H₂O(l)

A) UO₂(s) + 2HF(l) → UF₄(s) + H₂O(l)
B) UO₂(s) + 4HF(l) → UF₄(s) + 2H₂O(l)
C) UO₂(s) + H₄F₄(l) → UF₄ (s) + H₄O₂(l)
D) UO₂(s) + 4HF(l) → UF₄(s) + 4H₂O(l)
E) UO₂(s) + 8HF(l) → 2UF₄(s) + 4H₂O(l)

F) B) and E)
G) A) and D)

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Question 22

Multiple Choice

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Aluminum oxide, Al₂O₃, 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 Al₂O₃.

A) 2.377 mol
B) 2.146 mol
C) 1.105 mol
D) 0.4660 mol
E) 0.4207 mol

F) None of the above
G) A) and B)

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Question 23

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Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

Which of the following samples has the most moles of the compound?

One mole of methane (CH₄) contains a total of 3 × 10²⁴ atoms.

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.

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl₃. What mass of chlorine gas is needed to react completely with 163 g of aluminum?

A compound of bromine and fluorine is used to make UF₆, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula.

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N₂(g) + 3H₂(g) → 2NH₃(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp, and textiles) . SO₂(g) + 2Cl₂(g) → SOCl₂(g) + Cl₂O(g) If 0.400 mol of Cl₂ reacts with excess SO₂, how many moles of Cl₂O are formed?

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g) → P₄O₆(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen. 4Al(s) + 3O₂(g) → 2Al₂O₃(s) A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00g/mol) is allowed to react. What mass of aluminum oxide ( = 101.96 g/mol) can be formed?

Sodium bromate is used in a mixture which dissolves gold from its ores. Calculate the mass in grams of 4.68 mol of sodium bromate.

Phosphorus pentachloride, PCl₅, 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 PCl₅.

A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?

Balance the following equation: C₈H₁₈O₃(l) + O₂(g) → H₂O(g) + CO₂(g)

What is the percent yield for the reaction PCl₃(g) + Cl₂(g) → PCl₅(g) If 119.3 g of PCl₅ (M = 208.2 g/mol) are formed when 61.3 g of Cl₂ ( = 70.91 g/mol) react with excess PCl3?

Balance the following equation: B₂O₃(s) + HF(l) → BF₃(g) + H₂O(l)

Household sugar, sucrose, has the molecular formula C₁₂H₂₂O₁₁. What is the percent of carbon in sucrose, by mass?

Analysis of a carbohydrate showed that it consisted of 40.0 % C, 6.71 % H, and 53.3 % O by mass. Its molecular mass was found to be between 140 and 160 amu. What is the molecular formula of this compound?