Q4:-Put a mark of true or false in front of the following statements and correct the error,if any.-1-In (Cathodic protection system) sacrificial anode, which is more voltage than themetal to be protected from corrosion2-In oxidation-reduction reactions solutions of strong acids, the oxygen ions are lessreduced than the liberated hydrogen ions.-Techniques Tafel extrapolation test are used in corrosion rate measurements toovercoming the disadvantages of the Linear polarization method4-A differential deration cell,corrosion take place nom electrode being thoroughlyaerated to another de aerated.5-Selective Leaching corrosion based on the more electrochemical component of an alloyis usually the element that is removed.6-Electrolytic Cells are Non-spontaneous redox reactions and convert the chemicalenergy to electric energy.7-Sour Corrosion term refer on corrosion due to gases which contain high concentrationsof CO₂ alone, and called sour gas, while acid gas, can refer to a gases containing highconcentration as H₂S,CO₂,HCL.HF.

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aerated to another de aerated. 5-Selective Leaching corrosion based on the more electrochemical component of an alloy is usually the element that is removed. 6-Electrolytic Cells are Non-spontaneous redox reactions and convert the chemical energy to electric energy.

aerated to another de aerated. 5-Selective Leaching corrosion based on the more electrochemical component of an alloy is usually the element that is removed. 6-Electrolytic Cells are Non-spontaneous redox reactions and convert the chemical energy to electric energy.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 115AE: The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making...

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A baby's spoon with an area of 6.25 cm2 is plated with silver from AgNO3 using a current of 2.00 A for two hours and 25 minutes. (a) If the current efficiency is 82.0%, how many grams of silver are plated? (b) What is the thickness of the silver plate formed (d=10.5g/cm3) ?
In theory, most metals should easily corrode in air. Why? A group of metals called the noble metals are relatively difficult to corrode in air. Some noble metals include gold, platinum, and silver. Reference Table 17-1 to come up with a possible reason why the noble metals are relatively difficult to corrode.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
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-.
Identify each statement as true or false. Rewrite each false statement to make it true. (a) Oxidation always occurs at the anode of an electrochemical cell. (b) The anode of a discharging voltaic cell is the site ofreduction and is negative. (c) Standard-state conditions for electrochemical cells are aconcentration of 1.0 M for dissolved species and a pressure of 1 bar for gases. (d) The potential of a voltaic cell does not change withtemperature. (e) All product-favored oxidation-reduction reactions have astandard cell potential Ecell, with a negative sign.
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Ochem help with prelab The experiment is attached and involves the reduction of a nitro group to an amine The Chemicals are: 200 mg of m-nitroacetophenone 400 mg of granular tin 4 mL of 6M hydrochloric acid 30% sodium hydroxide Need help with the prelab which requires... A. Write the balanced equations for both half-reactions of the redox and then the overall balanced redox equation B. Determine the limiting reagent and the theoretical yield of amine
In a historical industrial process Co(CO)4H is generated in-situ from CoI2, CO and H2O. By-products are CO2 and HI. Give the two relevant half-equations and then construct the full redox equation.
A thin circular-disk earring 4.00 cm in diameter is platedwith a coating of gold 0.25 mm thick from an Au³⁺ bath.(a) How many days does it take to deposit the gold on one sideof one earring if the current is 0.013 A (d of gold =19.3 g/cm³)?(b) How many days does it take to deposit the gold on both sidesof the pair of earrings?(c) If the price of gold is $320 per troy ounce (31.10 g), what is the total cost of the gold plating?
4. Determining electrolytic activity in a dilute solution. Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milliampere current. The time required to liberate 0.01 mol of H2 gas at the cathode is?
Two Copper strips were used to determine the effect of supporting electrolyte used on the change in mass. Three different experiments were conducted for 5mins where 0.5A current is applied throughout the experiment. In the first experiment two copper strips were immersed in 3.080g of Cu (NO3)2 dissolved in 25mL of DI water and tested for 5mins while applying current 0.5A. The weight of one copper strip act as an anode is taken before the reaction and after the reaction to calculate the change in mass due to different applied current. Same process is repeated with 25ml 0.5 M CuSO4 and25ml 0.5 M CuCl2 for 5 mins Using Faraday’s equation (Eq 1), calculate the theoretical mass and Compares the theoretical mass (mg) of copper and the actual mass deposited (obtained from the electrolysis, ∆m) by calculating the %error at different times. Discuss the observed results. Q = I x t = nFN Electrolyte Initial mass of anode (mg) Final mass of anode (mg) Cu (NO3)2 2941 2893…
Through a solution containing 34.69 mmol tetramethylammonium picrate per kg of solution, a current was sent for 1 h 50 min between a Ag anode and a Ag/AgCl cathode. The solution was then divided into three parts: anode, middle, and cathode solution. The anode solution weighed 31.238 g and contained 42.36 mmol picrate ion per kg; the cathode solution weighed 46.065 g and contained 29.51 mmol picrate ion per kg. The middle solution still contained 34.69 mmol tetramethylammonium picrate per kg of solution and no other kinds of ions. In a coulometer, connected in series, 63.41 mg silver had simultaneously precipitated. The organic ions do not react in this process. Find the transference number of the cation at the temperature of the experiment.,