Ask Question
30 October, 06:09

When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of and. in a certain experiment, 20.00 g iron metal was reacted with 11.53 g oxygen gas. after the experiment, the iron was totally consumed, and 3.78 g oxygen gas remained. calculate the amounts of and formed in this experiment?

+4
Answers (1)
  1. 30 October, 09:58
    0
    Given:

    initial mass of Fe = 20.0 g

    initial mass of oxygen gas = 11.53 g

    mass of oxygen remained = 3.78 g

    Solution:

    The chemical reaction is expressed as:

    4Fe + 3O2 - - > 2Fe2O3

    We first calculate the oxygen that is used in the reaction,

    Mass oxygen used = 11.53 g - 3.78 g = 7.75 g O2

    Moles O2 = 7.75 g O2 (1 mol / 32 g) = 0.2422 moles O2

    Moles Fe2O3 produced = 0.2422 moles O2 (2 mol Fe2O3 / 3 moles O2) = 0.1615 mol Fe2O3

    Mass Fe2O3 produced = 0.1615 mol Fe2O3 (159.7 g / 1 mol) = 25.79 g Fe2O3

    Therefore, the mass of ferrous oxide produced would be 45.79 g Fe2O3.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of and. in a certain experiment, 20.00 g iron ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers