Chemistry

posted by .

The reaction between solid sodium and iron(III) oxide is one in a series of reactions that inflates an automobile airbag.
6 Na(s) + Fe2O3(s) 3 Na2O(s) + 2 Fe(s)

If 171.0 g Na and 213.5 g Fe2O3 are used in this reaction, what is the mass of excess reactant that remains after the reaction is complete?

  • Chemistry -

    1. Write the equation and balance it. You need to write in an arrow so you can tell where the reactants end and the products start.
    2a. Convert 171.0 g Na to moles. moles = grams/molar mass.
    2b. Do the same for 213.6 g Fe2O3.
    3a. Using the coefficients in the balanced equation, convert moles Na to moles of ANY product. I would choose Fe.
    3b. Do the same for converting moles Fe2O3 to moles of ANY product but choose the SAME one you chose in 3a.
    3c. Likely you will have two different answers for the product; obviously, both can't be correct (unless they are the same). The correct answer is ALWAYS the smaller one and the reactant producing that smaller one is the limiting reagent. The other reagent, of course, is the excess reagent.
    4. Using the coefficients in the balanced equation, convert moles of the limiting reagent (now that you have it identified) to moles of the excess reagent and convert that to grams. grams = moles x molar mass. That will be number of grams of excess reagent used.
    5. You know the excess reagent. You know how many grams you had initially. Subtract the grams used to find the amount remaining.
    Post your work if you get stuck.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    The reaction between solid sodium and iron(III) oxide is one in a series of reactions that inflates an automobile airbag. 6 Na(s) + Fe2O3(s) 3 Na2O(s) + 2 Fe(s) If 171.0 g Na and 213.5 g Fe2O3 are used in this reaction, what is the …
  2. chemistry

    iron(III) oxide reacts with carbon monoxide gas to form solid iron metal and carbon dioxide gas: Fe2O3 + 3 CO --> 2 Fe + 3 CO2 If you begin the reaction with 84.34 g of iron(III) oxide and 68.87 g of CO, which reactant will be in …
  3. Chemistry

    in a blast furnace, iron(III) oxide is used to produce iron by the following (unbalanced) reaction: Fe2O3 + CO = Fe + CO2 a. if 4 kg Fe2O3 are available to react, how many moles of CO are needed?
  4. AP Chemistry, Chem, science

    Can anyone please help me with this problem?
  5. Chemistry

    Iron(III) oxide reacts with carbon monoxide gas to form solid iron metal and carbon dioxide gas: Fe2O3 + 3 CO --> 2 Fe + 3 CO2 If you begin the reaction with 84.34 g of iron(III) oxide and 68.87 g of CO, which reactant will be in …
  6. chemistry

    Iron(III) oxide reacts with carbon monoxide gas to form solid iron metal and carbon dioxide gas: Fe2O3 + 3 CO --> 2 Fe + 3 CO2 If you begin the reaction with 84.34 g of iron(III) oxide and 68.87 g of CO, which reactant will be in …
  7. Last Question Plz helppp:((im soo sleepy!!:(

    1)The reaction between solid sodium and iron(III) oxide, Fe2O3(s), is one in a series of reactions that occurs when an automobile air bag inflates. 6Na(s) + Fe2O3(s) -> 3Na2o(s) + 2Fe(s) If 100.0 g of iron(III) oxide are used in …
  8. Chemistry

    4Fe + 3O2 -> 2Fe2O3 + 1.65E3 kJ C) what is the enthalpy change for the formation of 23.6 g of iron(iii) oxide?
  9. Chemistry

     4Fe + 3O2 -> 2Fe2O3 + 1.65E3 kJ  C) what is the enthalpy change for the formation of 23.6 g of iron(iii) oxide?
  10. Chemistry

    Iron metal is formed during the reduction of iron(III) oxide: Fe2O3 + 3CO 2Fe + 3CO2 When 29.7 kg of Fe2O3 react with 17.8 kg of CO and 4.5 kg of Fe are recovered, what is the percent yield for the reaction?

More Similar Questions