Half-Reaction, Addic SolutionPotential, E (volts)-3.045L"(aq) + eLi()K'(ag) + e K(s)Rb (aq) + eRb()Ba (aq) +2e- Ba(s)Sr (ag) + 2 e Sr(s)Ca (aq) +2 e Ca(s)Na (aq) + e Na()Mg "(aq) +2 e → Mg)H(+2e 2H (1)AP"(aq) +3 e Al(s)-2.925-2.925-2.90-2.89-2.87-2.7143D2.37-2.251.66Z (aq) + 4 e Zr)-1.53ZAS6) + 2 e Zn(x) + S (a4)-1.44-1.21CASG) + 2 e >Cd() + $ (a)V (aq) +2e V©)L.I8Mn (aq) + 2e Mn(s)1.181.01FeSts)C"(aq) + 2e >Cr(«).Zn (aq)+ 2 e →Zn(x)Cr"2e Fe(s) S (aq)0.91-0.7630.74(aq)+ 3e Cris)HgS() + 2 H (a4) +2 H0 USg)Ga (aq) + eGas)0.720.530.492 CO.()+211 aq) +2e (COOLD em)FeCr" (aq) + Cr (aq)CF (aq) + 2 e Cde)Sefe)+2 11 (aq 2e HSe2eFet)一040.410.4040.400356TI aq+TIG):0.340.28Co (aq) 2 e Cos)N og) +2x Ni)(SaF (ag) teSafs) F Go)Agl) e0.150140.1260,0%0,0000.10 [References]Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells3+(a) Cr(s) | Cr (aq) || Pd (aq) | Pd(s)2+2124(b) Zn(s) | Zn (ag) || Co (ag) | Co(s)24(© Ca(s), Cds(s) | S (aq) || Sn (ag) | Su[s)

Answered: Image /qna-images/answer/71983d7e-2934-433f-85d7-27458a04dea2.jpg

Answered: [References] Using values from the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Pt(s) | H,(g, 0.703 atm) | H* (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H¹ (aq) + 2e H₂(g) Cd²+ (aq) + 2 e¯ → Cd(s) D Calculate the H concentration. [H+] = Eº = 0.00 V Eº = -0.403 V M
When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of Oz is 2.21 atm, [K2Cr2O7) = 0.642 M, the [Cr3+] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(g) + Cr3+ *(aq) → H202(aq) + Cr20-2" (aq)
Calculate the cell potential at 25oC for the Cr(s) | Cr3+(aq) || Sn2+(aq) | Sn(s) electrochemical cell if the concentration of Cr3+(aq) is 0.50 M and the concentration of Sn2+(aq) is 0.090 M. Report your answer to 3 significant figures.
Calculate ΔG° for the redox reaction represented by the cell diagram Pt(s) | Cl2(g, 1 atm) || ZnCl2(aq, 1 M) | Zn(s).
9) At 25°C, what is the potential and the cell reaction for the following cell: Ni | Ni2+ (aq, 0010 M) || Cl(aq, 0.20M) | Cl2 (g, 1 atm) | Pt? What is the Keg at 298K?
Pt(k)| Fe³+(aq), Fe²+(aq) // I-(aq) | 12(k) | Calculate the standard cell potential for the Pt(k) Cell and interpret whether the reaction taking place in the cell will proceed spontaneously under standard conditions. E° (Pt|Fe³+, Fe²+) = 0.77 V . E°( 12 | I-) = 0.53 V
Mn(s)|Mn2+(aq)||Cr3+(aq)| Cr(s) Calculate the cell potential at 25oC if the concentration of Mn2+(aq) is 2.40 M and the concentration of Cr3+(aq) is 0.500 M. Report your answer to 3 significant figures. Use theStandard Reduction Potentials Table as needed.
Determine the cell potential for the following cell Zn(s) | Zn2+(aq), 0.500 M || Ag+(aq), 0.010 M | Ag(s) The standard reduction potentials of Zn2+(aq) and Ag+(aq) are –0.76 V and +0.80 V, respectively. A. 1.45 V B. 1.67 V C. 1.56 V D. 1.51 V E. 1.61 V
3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half- cell: Pt(s) | H2 (g, 1.0 bar) | H+(aq, 1.0 mol L-1) | Au3+(aq, ? mol L-1) | Au(s) What is the concentration of Au3+ in the solution if is Ecell is 1.24 ? Express your answer using two significant figures and don't include the exponent (e.g. if your answer is 2.5×10-4, only write 2.5)
For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M), Cr2+(aq)(.301M)|Pt(s) Determine the cell potential for this electrochemical cell by first calculating the standard cell potential and then by using the Nernst equation.
2. Calculate the cell potential for the cell below at 25 °C Ti(s) Ti(NO3)2(aq) (0.92 M)|| HgCl₂(aq) (0.43 M)|Hg(1)|

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[References] Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells 3+ 2+ (a) Cr(s) | Cr (aq) || Pd (aq) | Pd(s) 21 (b) Zn(s) | Zn (ag) || Co (aq) | Co(s) 24 (0 ca(s), Cds()|S (aq) || Sn (aq) | Su(s)