How would you balance the following equation: Fe+O2 --> Fe2O3?

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How would you balance the following equation: Fe+O2 --> Fe2O3?

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Answer 1 · 2015-11-02T06:48:40

$4 F e$ $4Fe$ + $3 O_{2}$ $3O_2$ $\to$ $rarr$ $2 F e_{2} O_{3}$ $2Fe_2O_3$

Explanation:

Step 1: Tally the number of atoms based on subscript.

$F e$ $Fe$ + $O_{2}$ $O_2$ $\to$ $rarr$ $F e_{2} O_{3}$ $Fe_2O_3$ (unbalanced)

left side: Fe = 1; O = 2
right side: Fe = 2; O = 3

Step 2: Start balancing the simple molecules first, in this case the $O_{2}$ $O_2$

$F e$ $Fe$ + $3 O_{2}$ $color (green) 3O_2$ $\to$ $rarr$ $F e_{2} O_{3}$ $Fe_2O_3$

left side: Fe = 1; O = 2 x $3$ $color (green) 3$ = 6
right side: Fe = 2; O = 3

Since there are now 6 $O$ $O$ atoms on the left, there must also be 6 $O$ $O$ atoms on the right. Notice that the right hand is one big molecule so whatever coefficient you would use to balance the $O$ $O$ atoms, you would also need to apply to the bonded $F e$ $Fe$ atom.

$F e$ $Fe$ + $3 O_{2}$ $3O_2$ $\to$ $rarr$ $2 F e_{2} O_{3}$ $color (red) 2Fe_2O_3$

left side: Fe = 1; O = 2 x 3 = 6
right side: Fe = 2 x $2$ $color (red) 2$ = 4; O = 3 x $2$ $color (red) 2$ = 6

Step 3: Now balance the rest of the equation.

$4 F e$ $color (blue) 4Fe$ + $3 O_{2}$ $3O_2$ $\to$ $rarr$ $2 F e_{2} O_{3}$ $2Fe_2O_3$

left side: Fe = 1 x $4$ $color (blue) 4$ = 4; O = 2 x 3 = 6
right side: Fe = 2 x 2 = 4; O = 3 x 2 = 6

The equation is now balanced.

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How would you balance the following equation: Fe+O2 --> Fe2O3?

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