Correct Let's calculate the number of moles of each reactant: 1 mol CH4 1370 g CH4X = 85.4 mol CH, 16.04 g CH4 1 mol H20 18.02 g H20 1280 g H,0 x = 71.0 mol H20 Now compare the number of moles of the reactants, taking into account the fact that each mole of CH4 requires 1 mole of H20 to react completely: 71.0 mol H2 O 0.832 mol H20 85.4 mol CH, 1 mol CH4 1 mol H20 1 mol CH4 0.832 mol H2 O 1 mol CH4 So, H20 is the limiting reactant. b what is the maximum mass of H2 that can be prepared? Mass = g H2 Submit

Correct Let's calculate the number of moles of each reactant: 1 mol CH4 1370 g CH4X = 85.4 mol CH, 16.04 g CH4 1 mol H20 18.02 g H20 1280 g H,0 x = 71.0 mol H20 Now compare the number of moles of the reactants, taking into account the fact that each mole of CH4 requires 1 mole of H20 to react completely: 71.0 mol H2 O 0.832 mol H20 85.4 mol CH, 1 mol CH4 1 mol H20 1 mol CH4 0.832 mol H2 O 1 mol CH4 So, H20 is the limiting reactant. b what is the maximum mass of H2 that can be prepared? Mass = g H2 Submit

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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