The reactions that take place at the cathode and the anode when 1.0 M solution of NiBr 2 , AlF 3 and MnI 2 is electrolyzed. Concept introduction: The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions. To determine: The reactions that take place at the cathode and the anode when 1.0 M solution of NiBr 2 is electrolyzed. The reaction taking place at cathode is, Ni 2 + + 2 e − → Ni E ° red = − 0.23 V The reaction taking place at anode is, 2 Br − → Br 2 + 2 e − E ° ox = − 1.09 V
The reactions that take place at the cathode and the anode when 1.0 M solution of NiBr 2 , AlF 3 and MnI 2 is electrolyzed. Concept introduction: The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions. To determine: The reactions that take place at the cathode and the anode when 1.0 M solution of NiBr 2 is electrolyzed. The reaction taking place at cathode is, Ni 2 + + 2 e − → Ni E ° red = − 0.23 V The reaction taking place at anode is, 2 Br − → Br 2 + 2 e − E ° ox = − 1.09 V
Solution Summary: The author explains the non-spontaneous reaction in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal.
Definition Definition Process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state.
Chapter 17, Problem 111E
(a)
Interpretation Introduction
Interpretation:
The reactions that take place at the cathode and the anode when
1.0M solution of
NiBr2,
AlF3 and
MnI2 is electrolyzed.
Concept introduction:
The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions.
To determine: The reactions that take place at the cathode and the anode when
1.0M solution of
NiBr2 is electrolyzed.
The reaction taking place at cathode is,
Ni2++2e−→NiE°red=−0.23V
The reaction taking place at anode is,
2Br−→Br2+2e−E°ox=−1.09V
(b)
Interpretation Introduction
Interpretation:
The reactions that take place at the cathode and the anode when
1.0M solution of
NiBr2,
AlF3 and
MnI2 is electrolyzed.
Concept introduction:
The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions.
To determine: The reactions that take place at the cathode and the anode when
1.0M solution of
AlF3 is electrolyzed.
The reaction taking place at cathode is,
2H2O+2e−→H2+2OH−E°red=−0.83V
The reaction taking place at anode is,
2H2O→O2+4H++4e−E°ox=−1.23V
(c)
Interpretation Introduction
Interpretation:
The reactions that take place at the cathode and the anode when
1.0M solution of
NiBr2,
AlF3 and
MnI2 is electrolyzed.
Concept introduction:
The non-spontaneous reaction takes place in an electrolytic cell in which there occurs conversion of electrical energy into chemical energy and this is used for the electrolysis of a metal. The electrolytic cell involves a cathode and an anode, both dipped into an electrolytic solution having both the positive and negative ions.
Using the following two half-reactions, determine the pH range in which $NO_2^-\ (aq)$ cannot be found as the predominant chemical species in water.* $NO_3^-(aq)+10H^+(aq)+8e^-\rightarrow NH_4^+(aq)+3H_2O(l),\ pE^{\circ}=14.88$* $NO_2^-(aq)+8H^+(aq)+6e^-\rightarrow NH_4^+(aq)+2H_2O(l),\ pE^{\circ}=15.08$
Indicate characteristics of oxodec acid.
What is the final product when hexanedioic acid reacts with 1º PCl5 and 2º NH3.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell