chemistry

Can some one please balance this equation for me
Fe + O2---> Fe2O3.

Fe + O2 ==> Fe2O3.
Here is the way to balance these equations by inspection, meaning, by trial and error.
Rule #1. You may not change any subscripts. Equations are balanced by changing ONLY the coefficients.
Look on the right side and I see 2 Fe atoms. So we move to the left and place a 2 in front of the Fe.
2Fe + O2 ==> Fe2O3

Now look at the 3 O on the right. That is what we must have on the left. Two ways to approach this. I can balance it by placing 3/2 in front of the O2 like this.
2Fe + 3/2 O2 ==> Fe2O3. And the equation balances. Let's check it.
We have 2 Fe atoms on the left and right.
We have 3 O (3/2 * 2 = 3) atoms on the left and right.
Most of us like to see equations in whole numbers, not fractions, so we now multiply the entire equation by 2 to get rid of the 1/2.
4Fe + 3O2 ==> 2Fe2O3.

The second way: Starting with
2Fe + O2 ==> Fe2O3.

Look at O on the right and there are 3 atoms with two O atoms on the left. We know a whole numbrer coefficient won't work, so we trial and error. Knowing that 6 is a multiple of both 2 and 3, we just multiply Fe2O3 by 2 in order to have 6 O atoms on the right. And on the left we have a coefficient of 3 for O2.
2Fe + 3O2 ==> 2Fe2O3.
That gives us 6 O on the left and 6 on the right. Of course, it messed up the Fe but we can fix that easily. Since we now have 4 Fe on the right, we change the 2 for 2Fe on the left to 4Fe and the final equation is
4Fe + 3O2 ==> 2Fe2O3.

If your algebra is up to speed the balancing can also be done this way:

Fe + xO2 ==> yFe2O3

balancing Fe atoms
1=2y------------------(1

balancing O atoms
2x=3y------------------(2

for from equation (1
y=1/2

and substituting this in equation (2

2x=3(1/2)

so x=3/4

Replacing the symbols in the original

Fe + 3/4O2 ==> 1/2Fe2O3

but we are not allowed fractions so multiply through by 4

4Fe + 3O2 ==> 2Fe2O3

  1. 👍
  2. 👎
  3. 👁
  1. Ag+
    N2==>Ag3N

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry ( stoichiometry )

    How many grams of iron can be made from 16.5g of Fe2O3 by the following equation: Fe2O3 + 3 H2 -----> 2 Fe + 3 H2O.

  2. Chemistry

    Fe2O3(s) + 2Al(s)-> 2Fe(l) + Al2O3(s) What is the theoretical yield of iron if we begin the reaction with 10.5 g of Al (assume an excess of Fe2O3)

  3. Chemistry

    I am having a bit of difficulty getting the net equation and the net ionic equation and the net ionic equation. I think I have the balance equation right. Thanks in advance for any help. For the acid base neutralization reaction

  4. Chemistry

    How many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7gFe? Fe2O3(s) + 3CO(g) => 3CO2(g) + 2Fe(s)

  1. Chemistry

    Sulfur dioxide is used to make sulfuric acid. one method of producing it is by roasting mineral sulfides, for example, FeS2(s) + O2 (g) ---> SO2(g) + Fe2O3(s) (unbalanced). A production error leads to the sulfide being placed in a

  2. Chem

    Calculate the number of grams of Fe formed when 0.300kg of Fe2O3 reacts. Equation: Fe2O3+CO-->Fe+CO2 converted .300kg to 300g Balanced Fe2O3+3CO-->2Fe+3CO2 So I started by trying this: 300gFe2O3(1molFe2O3/159.687gFe2O3)...and then

  3. Chem

    f 147 grams of FeS2 is allowed to react with 88 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

  4. Chemistry

    An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: αFe2O3(s)+βCO(g)→γFe(s)+δCO2(g) A)Balance this equation. B)Calculate the number of grams of CO that can react

  1. chemistry 2

    the balanced equation for the reduction of iron ore to the metal using CO is Fe2O3+3CO(g) -> 2Fe+3CO so what is the maximum of iron in grams that can bbe obtained from 454g (1.00 lb) of iron (III) oxide? AND what mass of CO is

  2. chemistry

    Iron(III) oxide can be reduced to metallic iron by heating it in the presence of carbon. Balance the following equation, then determine the ratio of C to Fe in the reaction? Fe2O3 + C → Fe + CO2?

  3. Chemistry

    Calculate the volume of CO2 that would be produced from 0.5 mole of Fe2O3 according to the equation.Fe2O3(s)+3CO(g)=2Fe(s)+3CO2(g). (1mole of a gas occupies 22.4dm3 at s.t.p)

  4. Chemistry

    A sample weighing 3.064 g is a mixture of Fe2O3 (molar mass = 159.69) and Al2O3 (molar mass = 101.96). When heat and a stream of H2 gas is applied to the sample, the Fe2O3 reacts to form metallic Fe and H2O(g). The Al2O3 does not

You can view more similar questions or ask a new question.