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Balance each redox reaction using the half-reaction method.(a) Zn(s) + Sn2+ (aq) ? Zn2+

Chapter 16, Problem 62P

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QUESTION:

Balance each redox reaction using the half-reaction method.

(a) \(\mathrm{Zn}(s)+\mathrm{Sn}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Sn}(s)\)

(b) \(\mathrm{Mg}(s)+\mathrm{Cr}^{3+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cr}(s)\)

(c) \(\mathrm{Al}(s)+\mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+\mathrm{Ag}(s)\)

Equation Transcription:

Text Transcription:

Zn(s)+Sn^{2+}(aq) rightarrow Zn^{2+}(aq)+Sn(s)

Mg(s)+Cr^{3+}(aq) rightarrow Mg^{2+}(aq)+Cr(s)

Al(s)+Ag+(aq) rightarrow Al^{3+}(aq)+Ag(s)

Questions & Answers

QUESTION:

Balance each redox reaction using the half-reaction method.

(a) \(\mathrm{Zn}(s)+\mathrm{Sn}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Sn}(s)\)

(b) \(\mathrm{Mg}(s)+\mathrm{Cr}^{3+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cr}(s)\)

(c) \(\mathrm{Al}(s)+\mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+\mathrm{Ag}(s)\)

Equation Transcription:

Text Transcription:

Zn(s)+Sn^{2+}(aq) rightarrow Zn^{2+}(aq)+Sn(s)

Mg(s)+Cr^{3+}(aq) rightarrow Mg^{2+}(aq)+Cr(s)

Al(s)+Ag+(aq) rightarrow Al^{3+}(aq)+Ag(s)

ANSWER:

Problem 62P :

Step 1:

Here, we have to balance each redox reaction using the half-reaction method :

Half reaction is either the oxidation or the reduction reaction of a redox reaction.

Steps to balance redox reaction using the half reaction method :

  1. First, we assign oxidation states to all atoms and then identify the substances that are being oxidized and reduced.
  2. Then we separate the overall reaction into two half-reactions - oxidation and reduction.
  3. Next, we balance each half-reaction with respect to mass in the following order :
  •  Balance all elements other than H and O.
  •  Balance O by adding H2O.
  •  Balance H by adding H+.
  1. Next, we balance each half-reaction with respect to charge by adding electrons to the right side of the oxidation half-reaction and the left side of the reduction half-reaction, making the sum of the charges on both sides of each equation equal.
  2. Next, we equal the number of electrons in both half-reactions by multiplying one or both half-reactions by a small whole number.
  3. Then we add the two half-reactions together, canceling electrons and other species as necessary.
  4. Finally we verify that the reaction is balanced with respect to both mass and charge.

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