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Exam 3: Stoichiometry: Ratios of Combination

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Question 41

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

A) 26.7%
B) 33.3%
C) 41.4%
D) 42.1%
E) 51.4%

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Question 42

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How many grams are contained in a 0.183 mol sample of ammonium phosphate?

A) 1.23 × 10^-3 g
B) 617 g
C) 20.7 g
D) 27.3 g
E) 815.1 g

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Question 43

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Which of the following substances contains the greatest mass of carbon?

What is the empirical formula for a sample containing 81.70% carbon and 18.29% hydrogen?

What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V₂O₅ with 40.0 g of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na₃(CO₃) (HCO₃) ·2H₂O. 2Na₃(CO₃) (HCO₃) ·2H₂O(s) → 3Na₂CO₃(s) + CO₂(g) + 5H₂O(g) When 1.00 metric ton (1.00 × 10³ kg) of trona is decomposed, 0.650 metric ton of Na₂CO₃ is recovered. What is the percent yield of this reaction?

What is the average mass, in grams, of one arsenic atom? (N_A = 6.022 × 10²³ mol^-1)

How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to produce lead(II) chloride and nitric acid?

Balance the following equation: Ca₃(PO₄) ₂(s) + SiO₂(s) + C(s) → CaSiO₃(s) + CO(g) + P₄(s)

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

What is the molar mass of nicotine, C₁₀H₁₄N₂?

What is the percent sulfur in iron(III) sulfate?

Calculate the molecular mass of tetraphosphorus decaoxide, P₄O₁₀, a corrosive substance which can be used as a drying agent.

What is the coefficient of O₂ when the following equation is properly balanced with the smallest set of whole numbers? ________ CH₃OH + ________ O₂ → ________ CO₂ + ________ H₂O

Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of aluminum, in uranium processing, and in the frosting of light bulbs) . 2NH₃(g) + 5F₂(g) → N₂F₄(g) + 6HF(g) How many moles of NH₃ are needed to react completely with 13.6 mol of F₂?

A compound was discovered whose composition by mass is 85.6% C and 14.4% H. Which of these formulas could be the molecular formula of this compound?

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

What is the coefficient of O₂ when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ________ C₁₈H₃₆O₂ + ________ O₂ → ________ CO₂ + ________ H₂ O

Hydroxylammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. What is its empirical formula?

What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine by mass?