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Chapter 4: 4.7 (page 173)

In an acidic solution hydrogen peroxide reacts with Fe+2 to produce Fe+3 and water. Write a balanced equation for this reaction.

Short Answer

Expert verified

Answer

The balanced equation will be

\({H_2}{O_2}\left( {aq} \right) + 2{H^ + }\left( {aq} \right) + 2F{e^{2 + }}\left( {aq} \right) \to 2{H_2}O\left( l \right) + 2F{e^{3 + }}\)

Step by step solution

01

Writing half-reaction

The oxidation half-reaction is:\(F{e^{2 + }}\left( {aq} \right) \to F{e^{3 + }}\left( {aq} \right) + {e^ - }\)

The reduction half-reaction is: \(2{H^ + }\left( {aq} \right) + 2{e^ - } \to 2{H_2}O\left( l \right)\)

02

Balancing the equation

The oxidation half-reaction is multiplied by 2 to balance the number of electrons:

\(2F{e^{2 + }}\left( {aq} \right) \to 2F{e^{3 + }}\left( {aq} \right) + 2{e^ - }\)

03

Adding both the equation

Adding both the oxidation and reduction half-reactions, the following was obtained:

\({H_2}{O_2}\left( {aq} \right) + 2{H^ + }\left( {aq} \right) + 2F{e^{2 + }} \to 2{H_2}O\left( l \right) + 2F{e^{3 + }}\left( {aq} \right)\)

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Most popular questions from this chapter

Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811MNaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration of sulfuric acid in this sample of rain?

Classify the following as acid-base reaction or oxidation-reduction reactions.

(a)\(N{a_2}S\left( {aq} \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}S\left( g \right)\)

(b)\(2Na\left( s \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}\left( g \right)\)

(c)\(Mg\left( s \right) + C{l_2}\left( g \right) \to MgC{l_2}\left( s \right)\)

(d)\(MgO\left( s \right) + 2HCl\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + {H_2}O\left( l \right)\)

(e)\({K_3}P\left( s \right) + 2{O_2}\left( g \right) \to {K_3}P{O_4}\left( s \right)\)

(f)\(3KOH\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to {K_3}P{O_4}\left( {aq} \right) + 3{H_2}O\left( l \right)\)

Write the net ionic equation representing the neutralization of any strong acid with an ionic hydroxide.
(Hint: Consider the ions produced when a strong acid is dissolved in water)

Write a balanced equation for the decomposition of ammonium nitrate to form molecular nitrogen, molecular oxygen and water. (Hint Balance oxygen last, since it is present in more than one molecule on the right side of the equation)

How many milliliters of a 0.1500-M solution of KOH will be required to titrate 40.00 mL of a 0.0656-M solution of H3PO4?

\({{\rm{H}}_3}{\rm{P}}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + 2KO}}{{\rm{H}}_{({\rm{aq}})}}{\rm{ }} \to {\rm{ }}{{\rm{K}}_2}{\rm{HP}}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + 2}}{{\rm{H}}_2}{{\rm{O}}_{({\rm{l}})}}\)
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