Question

Consider the reaction of hydrogen and oxygen to form water: 2H2 + O2 ? 2H2O (i) Which is the limiting reactant when 5.00 g of H2 and 10.0 g of O2 react? (ii) What is the maximum number of moles of H2O that can be formed? (iii) How many moles of the excess reagent remain unreacted? Show all calculations

          Consider the reaction of hydrogen and oxygen to form water:
2H2 + O2 ? 2H2O
(i) Which is the limiting reactant when 5.00 g of H2 and 10.0 g of O2 react?
(ii) What is the maximum number of moles of H2O that can be formed?
(iii) How many moles of the excess reagent remain unreacted?
Show all calculations

Consider the reaction of hydrogen and oxygen to form water:
2H2 + O2 ? 2H2O
(i) Which is the limiting reactant when 5.00 g of H2 and 10.0 g of O2 react?
(ii) What is the maximum number of moles of H2O that can be formed?
(iii) How many moles of the excess reagent remain unreacted?
Show all calculations

Added by Marcos T.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

05/31/2022

Step 1

The molar mass of H2 is approximately 2 g/mol and the molar mass of O2 is approximately 32 g/mol. So, 5.00 g of H2 is 5.00 g / 2 g/mol = 2.5 moles of H2 And, 10.0 g of O2 is 10.0 g / 32 g/mol = 0.3125 moles of O2 Show more…

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Consider the reaction of hydrogen and oxygen to form water: 2H2 + O2 -> 2H2O Which is the limiting reactant when 5.00 g of H2 and 10.0 g of O2 react? What is the maximum number of moles of H2O that can be formed? How many moles of the excess reagent remain unreacted? Show all calculations