Silver sulfide, the tarnish on silverware, comes from the reaction of silver metal with hydrogen sulfide (H₂S).The unbalanced equation is: Ag + H₂S + O₂ --> Ag₂S + H₂O Unbalanced If the reaction was used intentionally to prepare Ag₂S, how many grams would be formed from 496 g of Ag, 80.0 g of H₂S, and excess O₂ if the reaction takes place in 90% yield? (LO 3.9) (a) 525 g (b) 1139 g (c) 583 g (d) 1025

검증된 단계별 안내

Step 1: Balance the chemical equation. The balanced equation is: 4Ag + 2H₂S + O₂ --> 2Ag₂S + 2H₂O

Step 2: Calculate the number of moles of Ag and H₂S. Use the molar mass of Ag (107.87 g/mol) and H₂S (34.08 g/mol) to convert the given mass to moles.

Step 3: Determine the limiting reactant. The reactant that produces the least amount of product (Ag₂S) is the limiting reactant.

Step 4: Calculate the theoretical yield of Ag₂S. Use the stoichiometry of the balanced equation and the moles of the limiting reactant to calculate the moles of Ag₂S that can be formed. Then convert this to grams using the molar mass of Ag₂S (247.8 g/mol).

Step 5: Calculate the actual yield. The actual yield is 90% of the theoretical yield. Multiply the theoretical yield by 0.90 to get the actual yield.

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주요 개념

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using balanced chemical equations to calculate the amounts of substances consumed and produced. Understanding stoichiometry is essential for determining how much product can be formed from given amounts of reactants, especially when yields are less than 100%.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule. Knowing the molar mass of reactants and products is crucial for converting between grams and moles, which is necessary for stoichiometric calculations in chemical reactions.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated as the ratio of the actual yield to the theoretical yield, multiplied by 100. It indicates how much product was actually obtained compared to what was expected based on stoichiometric calculations. Understanding percent yield is important for evaluating the success of a reaction and for adjusting calculations when the yield is less than 100%.