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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