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Ch.4 - Chemical Quantities & Aqueous Reactions
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 52
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Chapter 4, Problem 52

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the limiting reactant and the theoretical yield.

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1
Write the balanced chemical equation for the reaction: \[ \text{SiO}_2 (s) + 2\text{C} (s) \rightarrow \text{Si} (l) + 2\text{CO} (g) \]
Convert the masses of \( \text{SiO}_2 \) and \( \text{C} \) to moles using their molar masses: \( \text{Molar mass of SiO}_2 = 60.08 \, \text{g/mol} \) and \( \text{Molar mass of C} = 12.01 \, \text{g/mol} \).
Calculate the moles of \( \text{SiO}_2 \) and \( \text{C} \) using the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \).
Determine the limiting reactant by comparing the mole ratio of \( \text{SiO}_2 \) to \( \text{C} \) from the balanced equation with the calculated moles.
Calculate the theoretical yield of silicon by using the moles of the limiting reactant and the stoichiometry of the balanced equation.
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Lead ions can be precipitated from solution with KCl according to the reaction: Pb2+ (aq) + 2 KCl(aq) → PbCl2(s) + 2 K+ (aq). When 28.5 g KCl is added to a solution containing 25.7 g Pb2+, a PbCl2 precipitate forms. The precipitate is filtered, dried, and found to have a mass of 29.4 g. Determine the percent yield for the reaction. Determine the theoretical yield of PbCl2. Determine the limiting reactant.
Textbook Question

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O2(g) → 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

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Textbook Question

Urea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2 NH3(aq) + CO2(aq) → CH4N2O(aq) + H2O(l) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

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Textbook Question

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the percent yield for the reaction.

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Textbook Question

Calculate the molarity of each solution.

c. 32.4 mg NaCl in 122.4 mL of solution

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Textbook Question

Calculate the molarity of each solution. a. 0.38 mol of LiNO3 in 6.14 L of solution b. 72.8 g C2H6O in 2.34 L of solution c. 12.87 mg KI in 112.4 mL of solution