1. Consider a cell buffered at pH 2.00 and consists of Fe²+ (aq) (0.004 M), Fe³+ (aq) (0.070 M) and MnO4 (aq) (0.024 M), Mn²+ (aq) (0.050 M), in which Fe²+ reduces MnO4 to Mn²+. a. Write the balanced reaction b. What is the standard cell potential? Is the cell galvanic or electrolytic? c. What is the actual cell potential at 35.0°C? reprinted with al Education nuna..

1. Consider a cell buffered at pH 2.00 and consists of Fe²+ (aq) (0.004 M), Fe³+ (aq) (0.070 M) and MnO4 (aq) (0.024 M), Mn²+ (aq) (0.050 M), in which Fe²+ reduces MnO4 to Mn²+. a. Write the balanced reaction b. What is the standard cell potential? Is the cell galvanic or electrolytic? c. What is the actual cell potential at 35.0°C? reprinted with al Education nuna..

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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1.Which of the following is an electrolytic cell? a.Pb(s)|Pb2+(aq)||Zn2+(aq)|Zn(s) b.Pt(s)|Fe2+(aq), Fe3+(aq)||MnO4-(aq), Mn2+(aq)|Pt(s) c.Co(s)|Co2+(aq)||Cu2+(aq)|Cu(s) d.Ni(s)|Ni2+(aq)||Cr2O72-(aq), Cr3+(aq)|Pt(s)2. The dissolution of NH4Cl in water is an endothermic process. If the initial temperature of water is 25°C, what is the expected final temperature of the aqueous system? a.higher than 25°C b.lower than 25°C c.half of 25°C d.still 25°C 3.If your base metal is Cr, which among the following metals can acts as a sacrificial anode for it? a.Cub.Mgc.Agd. Ni
Calculate the K and AG for the following reaction at 25 °C: Mg(s) + Pb2+(aq)=Mg2+(aq) + Pb (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Кс Part 2 of 2 G Round your answer to 4 significant digits. AG° kJ mol
What is the net reaction for the cell? Is it .44V or .22V?
Consider the following voltaic cell at 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? The overall cell reaction is Al3+(0.20 M, ag) Al3*(0.75 M, ag) and Ecell = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) AI3+(0.20 M, ag) and Ecell = +0.0113 V. None of these The overall cell reaction is Al3+(0.20 M, aq) Al3*(0.75 M, ag) and Ecell = +0.0113 V. There is no overall cell reaction and Ecell 0.00 V. %3D The overall cell reaction is Al3+(0.75 M, aq) Als*(0.20 M, aq) and Ecell = -0.0113 V.
Consider the voltaic cell diagrammed below: Pb (s)| Pb²+ (aq)l| H2 (g)| H* (aq) | Pt (s) a) Write the balanced chemical equation that occurs in the voltaic cell depicted in the diagram. b) If the concentration of Pb2+ in this cell is 0.035 M and the pH is 1.60, what pressure of H2 (g) would keep the cell reaction in equilibrium?
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
e. Calculate the cell potential Ecell of the Galvanic cell (25°C). Give your answer in volts (V).
A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 x 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2+ (aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ →Ag(s) E° = +0.8 V %3D O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12
4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.
1.Which of the following is an electrolytic cell? a.Pb(s)|Pb2+(aq)||Zn2+(aq)|Zn(s)b.Pt(s)|Fe2+(aq), Fe3+(aq)||MnO4-(aq), Mn2+(aq)|Pt(s)c.Co(s)|Co2+(aq)||Cu2+(aq)|Cu(s)d.Ni(s)|Ni2+(aq)||Cr2O72-(aq), Cr3+(aq)|Pt(s) 2. The dissolution of NH4Cl in water is an endothermic process. If the initial temperature of water is 25°C, what is the expected final temperature of the aqueous system? a.higher than 25°C b.lower than 25°C c.half of 25°C d.still 25°C3. What is the mineral formed when Cu corrodes to form a green coating on the surface? a.Cu(NO3)2 b.CuCO3 c.Cu2O d.Cu(OH)2
a. How many grams of NaCl is required to generate a 0.50 L 3.00M NaCl (aq) solution?b. Calculate the mass-percent NaCl in a 3.0 M NaCl (aq) solution with the density of 1.25kg / L? c. Draw the cell reaction for the galvanic cell that is described by the following cell-diagram:Al (s) │Al3+ (aq) ││Fe2+ (aq) │Fe (s)d. Decide the cell potential (Ecell) of the galvanic cell described in the cell diagram in Problem c when the concentrations are 0.100M for Fe2+ and 0.300M for Al3+ ?
Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś