The Latimer Diagram of Cr ions is show below0.551.342.10- 0.424- 0.90Cr,0 Cr(v) → Cr(iv) → Cr(1)Cr(11)Cr1.38- 0.74a.) What is the E° for the reduction of Cr2O,2 to Crt. Show your calculationb.)What is the E° for the reduction of CrO, to Cr** and Cr* to Cr**. Show your calculation.c.) From the given Latimer diagram construct a Frost diagram. Show your calculations andpredict what Cr species will undergo disproportion and predict the product of the reaction.

The Latimer diagram for Cr shows its standard reduction potentials from oxidation state +7 to 0. The…

The Latimer Diagram of Cr ions is show below 0.55 1.34 2.10 -0.424 - 0.90 Cr,0 → Cr{v) → Cr(Iv) Cr(1) → Cr[1) → Cr 1.38 - 0.74 a.) What is the E° for the reduction of Cr.O;2- to Cr*. Show your calculation b.)What is the E° for the reduction of CrzO,2- to Crt and Cr+ to Cr. Show your calculation. c.) From the given Latimer diagram construct a Frost diagram. Show your calculations and predict what Cr species will undergo disproportion and predict the product of the reaction.

The Latimer Diagram of Cr ions is show below 0.55 1.34 2.10 -0.424 - 0.90 Cr,0 → Cr{v) → Cr(Iv) Cr(1) → Cr[1) → Cr 1.38 - 0.74 a.) What is the E° for the reduction of Cr.O;2- to Cr*. Show your calculation b.)What is the E° for the reduction of CrzO,2- to Crt and Cr+ to Cr. Show your calculation. c.) From the given Latimer diagram construct a Frost diagram. Show your calculations and predict what Cr species will undergo disproportion and predict the product of the reaction.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 106QAP: In biological systems, acetate ion is converted to ethyl alcohol in a two-step process:...

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An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Repeat the directions for Question 106 using a cell constructed of a strip of nickel immersed in a 1.0-M Ni2+ solution and a strip of silver dipping into a 1.0-M Ag+ solution. Write the balanced chemical equation for the reaction that is product-favored. Calculate the cell potential. Draw a sketch of the cell and indicate the anode, cathode, and direction of electron flow.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?
The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.