Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold as this metal naturally has a yellow tone. If 1.91 g of rhodium is deposited at the cathode when a current of 6.65 A passes through an electrolytic cell for 1620 seconds, what is the oxidation state of rhodium in the aqueous solution? (MW of rhodium=102.91 g/mol; Faraday constant = 96485 C/mol e').

Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold as this metal naturally has a yellow tone. If 1.91 g of rhodium is deposited at the cathode when a current of 6.65 A passes through an electrolytic cell for 1620 seconds, what is the oxidation state of rhodium in the aqueous solution? (MW of rhodium=102.91 g/mol; Faraday constant = 96485 C/mol e').

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...

See similar textbooks

Similar questions

An electroplating process uses 15.0 A to chemically corrode (dissolve) a copper anode. What is the corrosion rate of the anode in grams per hour?
In the electrolysis of a 200 mL unknown metal solution, 0.0434 grams of cathode mass increases when a current of 0.50 A is passed through the cell for 5 minutes. Other experiments reveal that the metal has +2 valence. Which of the following is the metal in the electrolysis solution? (Pt: 195 g/mol; Si: 28,08 g/mol; Fe: 55,8 g/mol; Cd: 112,4 g/mol; Mn: 54,94 g/mol; 1 F : 96485 C)
75. Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should include a working electrode, a reference electrode, and a counter electrode. (B) The pH meter is unable to determine the pH of 0.1 M NaOH. (C) Silver chloride-coated silver wire is commonly used as a reference electrode in the pH meter. (D) The glass membrane must be hydrated. (E) The difference in potential between the inner and outer layers is the boundary potential.
A 10.0 gram sample of copper ore was dissolved in nitric acid and then electrolyzed until all of the copper(II) ion was extracted at the cathode as copper metal. If the electrolysis required 15.0 minutes at a current of 2.50 A's, determine the percentage of copper in the original ore sample?
In an electrochemical cell, a metal anode lost 0.286 g while a total volume of 0.04854 L of hydrogen gas was produced. The temperature was 298 K and the barometric pressure was 763.5 mm Hg. At 298 K, the vapor pressure of water is 23.8 mm Hg. What is the molar mass of the metal?
Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.
In one application, a 0.010-mm layer of chromium must be deposited on a part with a total surface area of 3.3 m2 from a solution of containing chromium(III) ions. How long would it take to deposit the layer of chromium if the current was 33.46 A? The density of chromium (metal) is 7.19 g/cm3.
what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52 h?
19.39
The decomposition of NaCl(l) into Na(l) and Cl2(g) is thermodynamically unfavorable. The decomposition requires the input of energy from an external source. The diagram represents an electrolytic cell that can be used to drive the decomposition reaction. Which of the following identifies a flaw in the representation? a) Oxidation is occurring at the anode. b) Molten Na is shown at the cathode. c) An external source of energy is not shown. d) The direction of the electron flow in the wires is incorrect.
What mass of rhodium (Rh) metal will be deposited from a solution of Rh3+ ions by running electrical current through the solution at 0.500 A for 120.0 minutes?
Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)