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Balance each redox reaction using the half-reaction method.(a) K(s) + Cr3+ (aq) ? Cr(s)
Chapter 16, Problem 61P(choose chapter or problem)
Balance each redox reaction using the half-reaction method.
(a) \(\mathrm{K}(s)+\mathrm{Cr}^{3+}(a q) \longrightarrow \mathrm{Cr}(s)+\mathrm{K}^{+}(a q)\)
(b) \(\mathrm{Mg}(s)+\mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Ag}(s)\)
(c) \(\mathrm{Al}(s)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+\mathrm{Fe}(s)\)
Equation Transcription:
Text Transcription:
K(s)+Cr^{3+}(aq) rightarrow Cr(s)+K^{+}(aq)
Mg(s)+Ag^{+}(aq) rightarrow Mg^{2+}(aq)+Ag(s)
Al(s)+Fe^{2+}(aq) rightarrow Al^{3+}(aq)+Fe(s)
Questions & Answers
QUESTION:
Balance each redox reaction using the half-reaction method.
(a) \(\mathrm{K}(s)+\mathrm{Cr}^{3+}(a q) \longrightarrow \mathrm{Cr}(s)+\mathrm{K}^{+}(a q)\)
(b) \(\mathrm{Mg}(s)+\mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Ag}(s)\)
(c) \(\mathrm{Al}(s)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+\mathrm{Fe}(s)\)
Equation Transcription:
Text Transcription:
K(s)+Cr^{3+}(aq) rightarrow Cr(s)+K^{+}(aq)
Mg(s)+Ag^{+}(aq) rightarrow Mg^{2+}(aq)+Ag(s)
Al(s)+Fe^{2+}(aq) rightarrow Al^{3+}(aq)+Fe(s)
ANSWER:
Problem 61P :
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 :
- First, we assign oxidation states to all atoms and then identify the substances that are being oxidized and reduced.
- Then we separate the overall reaction into two half-reactions - oxidation and reduction.
- 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+.
- 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.
- Next, we equal the number of electrons in both half-reactions by multiplying one or both half-reactions by a small whole number.
- Then we add the two half-reactions together, canceling electrons and other species as necessary.