Ask Question
14 June, 08:48

In the explosion of a hydrogen-filled balloon, 0.80 g of hydrogen reacted with 6.4 g of oxygen. How many grams of water vapor are formed? (Water vapor is the only product.)

+2
Answers (1)
  1. 14 June, 11:11
    0
    0.4 moles H2O x (18.0 g / mole) = 7.2 g H2O

    Explanation:

    write the values given in the question

    In an explosion of hydrogen balloon, 0.80g of hydrogen is reacted with 6.4g of oxygen.

    Write the balanced equation

    2 H2 + O2 - --> 2 H2O

    0.80 g H2 x (1 mole / 2g) = 0.4 moles H2

    6.4 g O2 x (1 mole / 32g) = 0.2 moles O2

    from balanced equation, 2 moles H2 react with 1 mole O2

    therefore

    0.4 moles H2 x (1 mole O2 / 2 moles H2) = 0.2 moles O2

    since we need 0.2 moles O2 to react with all the H2 and we have exactly that amount, the amounts are said to be

    "stoichiometric" and either reactant can be considered limiting

    from the balanced equation, 2 moles H2 - -> 2 moles H2O ... therefore

    0.4 moles H2 x (2 moles H2O / 2 moles H2) = 0.4 moles H2O

    Then

    0.4 moles H2O x (18.0 g / mole) = 7.2 g H2O
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “In the explosion of a hydrogen-filled balloon, 0.80 g of hydrogen reacted with 6.4 g of oxygen. How many grams of water vapor are formed? ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers