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Exam 3: Stoichiometry of Formulas and Equations

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Question 31

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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) $\rightarrow$ SOCl₂(g) + Cl₂O(g) If 0.400 mol of Cl₂ reacts with excess SO₂, how many moles of Cl₂O are formed?

A) 0.800 mol
B) 0.400 mol
C) 0.200 mol
D) 0.100 mol
E) 0.0500 mol

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Question 32

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Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus. What is its empirical formula?

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Question 33

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The number of hydrogen atoms in 0.050 mol of C₃H₈O₃ is

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

Aluminum sulfate, Al₂(SO₄) ₃, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.

How many molecules of molecular oxygen react with four molecules of NH₃ to form four molecules of nitrogen monoxide and six molecules of water?

How many grams of oxygen are needed to react completely with 200.0 g of ammonia, NH₃? 4NH₃(g) + 5O₂(g) $\rightarrow$ 4NO(g) + 6H₂O(g)

What will be the final volume of a solution prepared by diluting 25 mL of 8.25 M sodium hydroxide to a concentration of 2.40 M?

Methanol (CH₄O) is converted to bromomethane (CH₃Br) as follows: CH₄O + HBr $\rightarrow$ CH₃Br + H₂O If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield?

Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula?

The formula CH₃O_0.5 is an example of an empirical formula.

A 0.150 M sodium chloride solution is referred to as a physiological saline solution because it has the same concentration of salts as normal human blood. Calculate the mass of solute needed to prepare 275.0 mL of a physiological saline solution.

An important reaction sequence in the industrial production of nitric acid is the following: N₂(g) + 3H₂(g) $\rightarrow$ 2NH₃(g) 4NH₃(g) + 5O₂(g) $\rightarrow$ 4NO(g) + 6H₂O(l) Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?

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

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.

Balance the following equation: UO₂(s) + HF(l) $\rightarrow$ UF₄(s) + H₂O(l)

Magnesium reacts with iron(III) chloride to form magnesium chloride (which can be used in fireproofing wood and in disinfectants) and iron. 3Mg(s) + 2FeCl₃(s) $\rightarrow$ 3MgCl₂(s) + 2Fe(s) A mixture of 41.0 g of magnesium (? = 24.31 g/mol) and 175 g of iron(III) chloride (? = 162.2 g/mol) is allowed to react. What mass of magnesium chloride = 95.21 g/mol) is formed?

When 2.61 g of solid Na₂CO₃ is dissolved in sufficient water to make 250. mL of solution, the concentration of Na₂CO₃ is:

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

In combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO₂ and H₂O collected in the absorbers.