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Use 1 decimal point for all atomic masses. 2.00 g of H2(g) are reacted with 32.0 g of O2(g) by the following reaction   2H2(g) + O2(g) --> 2H2O(g) What is the limiting reagent? H2(g) O2(g)     Based on the limiting reagent, fill in the following ICE Table using moles. Enter any zero values as 0.00.     H2 O2 H2O Initial       Change       Final         How much of the excess reagent remains (in grams)?

Use 1 decimal point for all atomic masses. 2.00 g of H2(g) are reacted with 32.0 g of O2(g) by the following reaction   2H2(g) + O2(g) --> 2H2O(g) What is the limiting reagent? H2(g) O2(g)     Based on the limiting reagent, fill in the following ICE Table using moles. Enter any zero values as 0.00.     H2 O2 H2O Initial       Change       Final         How much of the excess reagent remains (in grams)?

World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 50A
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Use 1 decimal point for all atomic masses. 2.00 g of H2(g) are reacted with 32.0 g of O2(g) by the following reaction

 
2H2(g) + O2(g) --> 2H2O(g)
What is the limiting reagent?
H2(g)
O2(g)    
Based on the limiting reagent, fill in the following ICE Table using moles. Enter any zero values as 0.00.

 

  H2 O2 H2O
Initial      
Change      
Final      

 

How much of the excess reagent remains (in grams)?

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