Given are two half-cells, described by the equations: Zn^(2+)(aq) + 2e- -> Zn(s) E(standard) = -0.76 V Ag^(+)(aq) + e...
Given are two half-cells, described by the equations:
Zn^(2+)(aq) + 2e- -> Zn(s) E(standard) = -0.76 V
Ag^(+)(aq) + e- -> Ag(s) E(standard) = +0.80 V
A. Write down the net equation for the spontaneous reaction that
takes place in the cell.
B. Draw the two half cells and mark the anode and the
cathode.
C. Mark the solutions' concentration necessary in order to reach
the standard potential.
D. How will the cell's potential be influenced by the addition
of a KI-solution? Explain! (an AgI sediment is created)
E. What will be the cell's potential when the concentration of
solution Zn(NO3)2 will be 0.5 M and when the concentration of AgNO3
will be 0.4 M. Show calculations!
Homework Answers
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Given are two half-cells, described by the equations: Zn^(2+)(aq) + 2e- -> Zn(s) E(standard) = -0.76 V Ag^(+)(aq) + e...
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s)...
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
Question 17 1 pts Given these half cell reactions: Zn+2 (aq) + 2e → Zn (s)...
Question 17 1 pts Given these half cell reactions: Zn+2 (aq) + 2e → Zn (s) E = -0.76 V Ag+ (aq) + e Ag (s) E° = 0.80V Write the Cell Diagram (line notation) representing the anode and cathode half reactions. Note: Use forward slash as line separators, HTML Editor BIVA -A- IE * 3 1 1 x'x, EE D D N V VD 1 2pt - Paragraph - ®
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + €...
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
Consider the following reaction. 2Ag^+(aq) + Zn(s) --> 2Ag(s) +Zn(aq) a) write the individual oxidation and...
Consider the following reaction. 2Ag^+(aq) + Zn(s) --> 2Ag(s) +Zn(aq) a) write the individual oxidation and reduction half-reactions, specifying which is the anode and which is the cathode reaction. b) calculate the cell potential for a cell containing 0.10M Ag^+ and 0.25M Zn^2+ at 298K. (E ag= 0.80 V and E zn= -0.76 V)
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2:...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
half-reaction standard reduction potential Zn?" (aq)+2e" - Zn(s) Epod= -0.763 V MnO, (aq)+2 H,0(1+3e" - MnO,(s)+4...
half-reaction standard reduction potential Zn?" (aq)+2e" - Zn(s) Epod= -0.763 V MnO, (aq)+2 H,0(1+3e" - MnO,(s)+4 OH (aq). E = +0.59 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. X 5 ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written Yes Do you have...
Given: Zn2+ (aq) + 2e Zn(s); E--0.76 V Cu²+ (aq) +20 Cu(s); E° -0.34 V What...
Given: Zn2+ (aq) + 2e Zn(s); E--0.76 V Cu²+ (aq) +20 Cu(s); E° -0.34 V What is the cell potential of the following electrochemical cell at 25°C? Zn(s) | Zn2+(1.0 M) || Cu2+(0.0010 M) Cu(s) a) greater than 1.10 v b) between 0.76 and 1.10 V c) less than 0.42 V d) between 0.00 and 0.76 V e) between 0.34 and 0.76 V
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+...
The following half-cells are availble: (i) Ag+ (1.0 M) ∣ Ag (s) 0.7994 v (ii) Zn2+ (1.0 M) ∣ Zn (s) -0.76 v (iii) Cu2+ (1.0 M) ∣ Cu (s) 0.337 v (iv) Co2+ (1.0 M) ∣ Co (s) -0.28 v Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag - Zn, Ag-Cu, Ag-Co, Zn - Cu, Zn-Co, and Cu-Co. (the first metal is the anode...
Given the following half-cell potentials, i. Zn2+ + 2 e– → Zn (E° = –0.76 V)...
Given the following half-cell potentials, i. Zn2+ + 2 e– → Zn (E° = –0.76 V) ii. Cr3+ + 3 e– → Cr (E° = –0.74 V) determine the cell potential whose overall redox reaction under standard conditions is 3 Zn(s) + 2 Cr3+(aq) → 3 Zn2+(aq) + 2 Cr(s): * A. –0.80 V B. –0.02 V C. +0.02 V D. +0.80 V
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С
Question 17 1 pts Given these half cell reactions: Zn+2 (aq) + 2e → Zn (s) E = -0.76 V Ag+ (aq) + e Ag (s) E° = 0.80V Write the Cell Diagram (line notation) representing the anode and cathode half reactions. Note: Use forward slash as line separators, HTML Editor BIVA -A- IE * 3 1 1 x'x, EE D D N V VD 1 2pt - Paragraph - ®
Half-cell Potentials: Half Reaction: E value +0.80 V Agt + e → Ag Fe3+ + € → Fe2+ +0.77 v +0.34 V -0.13 V Cu2+ +2e → Cu Pb2+ + 2e - → Ib Ni2+ + 2e → Ni Cd2+ +2e → Cd -0.25 V -0.40 V Fe2+ + 2e → Fe -0.44 V Zn2+ + 2e → Zn -0.76 V Al3+ +3e → AI - 1.66 V Consider an electrochemical cell constructed from the following half cells, linked by...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
half-reaction standard reduction potential Zn?" (aq)+2e" - Zn(s) Epod= -0.763 V MnO, (aq)+2 H,0(1+3e" - MnO,(s)+4 OH (aq). E = +0.59 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. X 5 ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written Yes Do you have...
Given: Zn2+ (aq) + 2e Zn(s); E--0.76 V Cu²+ (aq) +20 Cu(s); E° -0.34 V What is the cell potential of the following electrochemical cell at 25°C? Zn(s) | Zn2+(1.0 M) || Cu2+(0.0010 M) Cu(s) a) greater than 1.10 v b) between 0.76 and 1.10 V c) less than 0.42 V d) between 0.00 and 0.76 V e) between 0.34 and 0.76 V
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