Question

In: Chemistry

Hydrogen gas is blown over hot iron (II) oxide. Write the balanced half reactions and the...

Hydrogen gas is blown over hot iron (II) oxide. Write the balanced half reactions and the balanced net ionic equation.

I know the half reactions are

H2 -> H2O and FeO -> Fe

But I don't understand how to get these. Why is the oxygen still with the iron in the half reaction? Thanks.

Solutions

Expert Solution

Note that we must "balance" this reaction

we can't simply get rid of FeO, since it is a solid, therefore

FeO --> Fe

H2 --> H2O

REDOX balancing

First, define the “ACIDIC” solution/conditions as H+ presence and

Basic solution implies OH- once it is balanced.

Also; note that ALL species must be balanced, as well as charges

Typical steps:

1) split half redox cells

2) balance atoms other than O,H

3) balance O by adding H2O

4) balance H by adding H+

5) balance charge by adding e-

6) balance e- by multiplying by the Greatest common divisor

7) Add both equations

8) simplify repeating elements, H+, H2O, and e- typically

9) add OH- if we need basic media, otherwise this is done.

10) Simplify again

FeO --> Fe

H2 --> H2O

balance O adding H2O

FeO --> Fe + H2O

H2O + H2 --> H2O

balance H adding H+

2H+ + FeO --> Fe + H2O

H2O + H2 --> H2O + 2H+

balance charge

2e- + 2H+ + FeO --> Fe + H2O

H2O + H2 --> H2O + 2H+ + 2e-

add all

H2O + H2 + 2e- + 2H+ + FeO --> Fe + H2O + H2O + 2H+ + 2e-

cnacel common terms

H2 + FeO --> Fe + H2O

therefore, this is the balanced reaction

it seems "simple" but in reality, we just ensured balance of: elements, O, H, Fe, and charge/electron balance


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