A 5.00 g sample of metallic copper (MW: 63.546) is reacted with an excess of oxygen gas (MW: 31.998). The reaction is given by the equation below. Cu(s) + O2(9) –→ CuO(s) Note: Use proper number of significant figures for succeeding questions. Balance the equation. Note: DO NOT USE FRACTIONS. USE THE LOWEST POSSIBLE SET OF COEFFICIENTS 2 |Cu(s) + 1 02 (g) CuO(s) Calculate the theoretical moles and mass of CuO(s) that will be produced from the reaction. moles of CuO theoretical : mol mass of CuO theoretical : g If 4.626 g of product was obtained from the reaction, calculate the yield. yield: %

A 5.00 g sample of metallic copper (MW: 63.546) is reacted with an excess of oxygen gas (MW: 31.998). The reaction is given by the equation below. Cu(s) + O2(9) –→ CuO(s) Note: Use proper number of significant figures for succeeding questions. Balance the equation. Note: DO NOT USE FRACTIONS. USE THE LOWEST POSSIBLE SET OF COEFFICIENTS 2 |Cu(s) + 1 02 (g) CuO(s) Calculate the theoretical moles and mass of CuO(s) that will be produced from the reaction. moles of CuO theoretical : mol mass of CuO theoretical : g If 4.626 g of product was obtained from the reaction, calculate the yield. yield: %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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[References] Copper metal can be prepared by roasting copper ore, which can contain cuprite (Cu₂ S) and copper(II) sulfide. Cu₂ S (s) + O2(g) → 2 Cu(s) + SO2(g) CuS(s) + O₂(g) → Cu(s) + SO2(g) Suppose an ore sample contains 12.0% impurity in addition to a mixture of CuS and Cu₂ S. Heating 100.0 g of the mixture produces 75.7 g of copper metal with a purity of 88.2%. What is the weight percent of CuS in the ore? The weight percent of Cu₂S? Weight percent of CuS = 2 Weight percent of Cu₂S: Submit Answer = % % Try Another Version 9 item attempts remaining Cengage Learning Cengage Technical Support Previous Next Save and Exit
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO (aq) → Cu(s) + FESO,(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 64. mg. Ar Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits. 10