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For the reaction above, if we start with 5.8 mol of hydrogen and 3.1 mol of oxygen, how many moles of water can be produced, and what remains unreacted?

For the reaction above, if we start with 5.8 mol of hydrogen and 3.1 mol of oxygen, how many moles of water can be produced, and what remains unreacted?

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question 3 H2 + 02 - H20 For the reaction above, if we start with 5.8 mol of hydrogen and 3.1 mol of oxygen, how many moles of water can be produced, and what remains unreacted? O a 3.1 moles of water would be produced, with 1.5 moles of O2 remaining. O b 5.8 moles of water would be produced, with 0.8 moles of O, remaining. 3.1 moles of water would be produced, with 0.8 moles of O, remaining. O d 5.8 moles of water would be produced, with 0.20 moles of O, remaining.
Transcribed Image Text:Question 3 H2 + 02 - H20 For the reaction above, if we start with 5.8 mol of hydrogen and 3.1 mol of oxygen, how many moles of water can be produced, and what remains unreacted? O a 3.1 moles of water would be produced, with 1.5 moles of O2 remaining. O b 5.8 moles of water would be produced, with 0.8 moles of O, remaining. 3.1 moles of water would be produced, with 0.8 moles of O, remaining. O d 5.8 moles of water would be produced, with 0.20 moles of O, remaining.
Expert Solution
Step 1

given:-

number of moles of H2 = 5.8 mol 

number of moles of O2 = 3.1 mol 

To calculate :- moles of H2O produced and number of moles of excess reactant remaining.

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