Balancing Redox Reaction Video Lessons

Concept

# Problem: Balance the following oxidation-reduction reaction:Fe(s) + Na+ (aq) → Fe2+ (aq) + Na(s) Express the coefficients as integers separated by commas (e.g., 4 ,1 ,3 ,2 where 1 indicates the absence of a coefficient).Balance the following oxidation-reduction reaction: K(s) + H2O(l) → KOH(aq) + H2(g) Express the coefficients as integers separated by commas (e.g., 4 ,1 ,3 ,2 where 1 indicates the absence of a coefficient).

###### FREE Expert Solution

Balance the redox reaction under acidic conditions: Fe(s) + Na+ (aq) → Fe2+(aq) + Na(s)

*Before balancing the redox reaction:

ignore H+, OH-, and H2O in the starting reaction

Step 1: Separate the whole reaction into half-reaction

Fe(s) → Fe2+(aq)                                                 Na+ (aq)  → Na(s)

Step 2: Balance the non-hydrogen and non-oxygen elements first

Fe(s) → Fe2+(aq)                                                 Na+ (aq)  → Na(s)

(Fe: balanced)                                                (Na: balanced)

Step 3: Balance oxygen by adding H2O(l) to the side that needs oxygen (1 O: 1 H2O)

Fe(s) → Fe2+(aq)                                                 Na+ (aq)  → Na(s)

(No oxygens)                                                   (No oxygens)

Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen (1 H: 1 H+)

Fe(s) → Fe2+(aq)                                                 Na+ (aq)  → Na(s)

(No hydrogens)                                              (No hydrogens)

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###### Problem Details

Balance the following oxidation-reduction reaction:

Fe(s) + Na+ (aq) → Fe2+ (aq) + Na(s)

Express the coefficients as integers separated by commas (e.g., 4 ,1 ,3 ,2 where 1 indicates the absence of a coefficient).

Balance the following oxidation-reduction reaction:

K(s) + H2O(l) → KOH(aq) + H2(g)

Express the coefficients as integers separated by commas (e.g., 4 ,1 ,3 ,2 where 1 indicates the absence of a coefficient).