A mixture of 6.00 g hydrogen (H2. molecular weight 2.016 g/mol) and 35.0 g oxygen (O2, molecular weight 31.998 g/mol) is prepared in an explosion-proof container, and allowed to react forming liquid water (H2O, 18.016 g/mol). 2 H2(g) + O2lg) ---> 2 H2O(1) This explosive reaction is known to have a nearly 100% yield, so it proceeds until all limiting reagent is used up. Please select the correct amount at the end of the reaction. 3.79 g H2 and 39.4 g H2O 3.79 g H2 and 53.6 g H2O 1.59 g H2 and 53.6 g H2O 3.79 g H2 and 26.8 g H2O 1.59 g H2 and 26.8 g H2O 1.59 g H2 and 39.4 g H2O

A mixture of 6.00 g hydrogen (H2. molecular weight 2.016 g/mol) and 35.0 g oxygen (O2, molecular weight 31.998 g/mol) is prepared in an explosion-proof container, and allowed to react forming liquid water (H2O, 18.016 g/mol). 2 H2(g) + O2lg) ---> 2 H2O(1) This explosive reaction is known to have a nearly 100% yield, so it proceeds until all limiting reagent is used up. Please select the correct amount at the end of the reaction. 3.79 g H2 and 39.4 g H2O 3.79 g H2 and 53.6 g H2O 1.59 g H2 and 53.6 g H2O 3.79 g H2 and 26.8 g H2O 1.59 g H2 and 26.8 g H2O 1.59 g H2 and 39.4 g H2O

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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