CH4(g) + 2 Cl2(g) → CH2C12(g) + 2 HCI(g) CH4 reacts with Cl2 as shown by the equation above. A chemist adds 1.35 moles of CH4 is placed in a reaction vessel containing 3.58 mol of Cl2(g). (a) Identify the limiting reactant. Justify your answer with a calculation. (b) Calculate the total number of moles of CH2CI2(g) in the container after the limiting reactant has been totally consumed. (c) Calculate the total moles of the excess reactant left over. (d) If 0.95 moles of CH,Cl, are produced in the lab, what is the percent yield?

CH4(g) + 2 Cl2(g) → CH2C12(g) + 2 HCI(g) CH4 reacts with Cl2 as shown by the equation above. A chemist adds 1.35 moles of CH4 is placed in a reaction vessel containing 3.58 mol of Cl2(g). (a) Identify the limiting reactant. Justify your answer with a calculation. (b) Calculate the total number of moles of CH2CI2(g) in the container after the limiting reactant has been totally consumed. (c) Calculate the total moles of the excess reactant left over. (d) If 0.95 moles of CH,Cl, are produced in the lab, what is the percent 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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