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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insert step 1> Write the balanced chemical equation for the reaction: SiO_2 (s) + 2C (s) -> Si (l) + 2CO (g).

insert step 2> Calculate the molar masses of SiO_2, C, and Si using the periodic table.

insert step 3> Convert the given masses of SiO_2 and C to moles using their respective molar masses.

insert step 4> Determine the theoretical yield of silicon by using stoichiometry based on the limiting reactant.

insert step 5> Calculate the percent yield using the formula: (actual yield / theoretical yield) * 100.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to determine the proportions of substances involved in a reaction, which is essential for predicting how much product can be formed from given amounts of reactants.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to the theoretical yield. It is expressed as a percentage and provides insight into how much of the expected product was actually obtained, helping to assess the effectiveness of the reaction conditions.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for accurate stoichiometric calculations and for determining the theoretical yield of the reaction.

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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.

Textbook Question

Calculate the molarity of each solution.

a. 3.25 mol of LiCl in 2.78 L solution

b. 28.33 g C₆H₁₂O₆ in 1.28 L of solution

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