43. Consider the voltaic cell: Fe(s) Salt bridge containing KNO3(aq) -1 M Fe³+ 1M Cr³+ Cr(s) a. Determine the direction of electron flow and label the anode and the cathode. b. Write a balanced equation for the overall reaction and calculate Ecell- c. Label each electrode as negative or positive. d. Indicate the direction of anion and cation flow in the salt bridge.

43. Consider the voltaic cell: Fe(s) Salt bridge containing KNO3(aq) -1 M Fe³+ 1M Cr³+ Cr(s) a. Determine the direction of electron flow and label the anode and the cathode. b. Write a balanced equation for the overall reaction and calculate Ecell- c. Label each electrode as negative or positive. d. Indicate the direction of anion and cation flow in the salt bridge.

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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2. Write the cell notation and cell diagram; and identify which is in anode and cathode. a. Ag+(aq) + Mg(s) ----> Ag(s) Mg(s) b. AgcI(s) + Fe(s) -----> Ag(s) + Fe+2(aq) + Cl- (aq) c. Fe(s) + H+(aq) -----> Fe+2(aq) + H2(g,1atm) d. Pb+2(aq) + Cr+2(aq) -----> Pb(s) + Cr+3(aq) e. Au+3(aq) + Fe+2(aq) -----> Au(s) + 4 Cl-(aq) + Fe+3(aq) f. K+(aq) + H2O(I) ----> 02(g) + H+ (aq) + K(s) a. Ag'ia + Mg --> Ag Mg b. AgClos + Fe -----> Aga) + Fe* + Clua) c. Fe + H'ag) > Fela + Hae latm d. Pb" + Cr e. Au f. K'ua + HOn > On + H'aa) + Ko --> Pb + Cru -> Au + 4 Cl n) + Fe" + Fe 2. For the above item #1, a-f; write the cell notation and cell diagram; and identify which is in anode and cathode.
4. Consider the voltaic cell: Pb(s) Cla(g) Salt bridge containing NANO;(aq) -1M Pb+ 1M C a. Determine the direction of electron flow and label the anode and the cathode. b. Write a balanced equation for the overall reaction and calculate Ee c. Label each electrode as negative or positive. d. Indicate the direction of anion and cation flow in the salt bridge.
Given the following electrochemical cell, from which of the listed compounds or elements is the anode made? Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Select one: a. Cu2+(aq) b. Ag(s) c. Ag+(aq) d. Cu(s)
please help
Using a table of standard electrode potentials, decide which of the following statements is completely true. Multiple Choice H* can oxidize Fe, and Ni can reduce Brz. Ni2" can oxidize Cu?", ond Fo2" can reduce H". O Cu2" can oxidize H2, and Fe can reduce Mn2". Br2 can oxidize Ni, and H2 can reduce Mn2 Fe" can oxidize H2, and Fe" can reduce Au".
Using a table of standard electrode potentials, decide which of the following statements is completely true. Multiple Choice cu2" can oxidize H2, and Fe can reduce Mn2". H* can oxidize Fe. and NI can reduce Br2. Ni2" can oxidize Cu?", and Fe2* can reduce H". Fe?" can oxidize H2, and Fe2“ can reduce Au3". Br2 can oxidize NI, and H2 can reduce Mn*.
11. The following two half-cells are connected to form a full Galvanic cell: Cu"(aq) +2e Au (aq) +e → Cu(s) → Au(s) E° = 0.34 V E 1.69 V a. Calculate E° for the cell. b. Give the cell notation for this system. c. Give the balanced cell reaction. d. Calculate AG for the reaction e. Calculate Keg for the reaction. £. Calculate the cell potential if the activity of Cu is 0.0100 and the activity of Au" is 1.340.
9. A voltaic cell is constructed using the following: Fe (s) + 2H* (aq) -> H2 (g) + Fe (aq) a. What is the potential under standard conditions? b. What is the potential when [Fe2] = 1.25 M, P2 = 1.15 atm, and the pH in both cells is 4.75 at 298 K? C. What is the Gibb's Free Energy and the equilibrium constant, K under standard conditions? What are these values with the conditions of part b? Did the reaction become more or less spontaneous? Explain.
As with any voltaic cell, the potential of zinc-copper cell changes during cell operation because the concentrations of the components do.If E°cell = + 2.71 V, [Mg2+] = 1.0 x 10-4 M and [Cu2+] = 2.0 M; find Ecell.Is the reaction at equilibrium?
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2. Draw a diagram for the following standard cell (3 mks): a. Label the following: Ag(s) 1 Ag (aq) Il Cu²+(aq) 1 Cu(s) Electrodes: cathode or anode; positive or negative Electrolytes direction of electron flow direction of ion movement.
14. In a electrochemical cell, metal D can displace Fe?"(aq) but not Mg"(aq). Identify the metal D. D2* (aq) + 2e → D (s) Reduction Half-Reaction V E° red -1.66 3+ Al (aq) + 3e¯ -→ Al (s) 24+ Са (ag) + 2е -> Са (s) 2+ Cu (aq) + 2e → Cu (s) -2.87 +0.34 2+ -0.44 Fe (aq) + 2e → Fe (s) 2+ -2.37 Mg (aq) + 2e Mg (s) 2+ -0.76 Zn (aq) + 2e → Zn (s) A. Al В. Са С. Си D. Zn