Answered: Analytical Chemistry II Why is carbon…

Science

Chemistry

Analytical Chemistry II Why is carbon used as an electrode in arc and spark sources? Explain briefly

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.4QAP

See similar textbooks

Related questions

Q: The following potential diagram summarizes the results of electrochemical studies of the aqueous…

A: The reduction potential of ClO4- to Cl2 will be the change of total reduction potential of every…

Q: Based on standard reduction potentials, would you expect copper metal to oxidize under standard…

A: The value of E˚cell is calculated as shown below: Here, E cell is the standard potential of the…

Q: How many grams of chromium metal can be deposited using an electrolytic cell with an electrolyte…

A: Given : Current = 8.30 A Time = 6 min = 6 X 60 s = 360 s And the salt given is CrCl3.

Q: Calculate the standard potential of Ni*/Ni electrode, if the cell potential of the cell…

A: Cell reaction:

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCla, it %3D deposits on…

A: Molar mass of gold is :- 197g/mol It is needed to deposit 0.40g of Au Current passed = 0.10 A

Q: A concentration cell similar to the one shown is composed of two Mg electrodes and solutions of…

A: Oxidation is lose of electrons. Reduction is gain of electrons. Reactions where oxidation and…

Q: For the reaction: Pd2+ + Ni → Ni²+ + Pd , AG° is –239 kJ/mole. What is the standard reduction…

A: The tendency possessed by ions to get reduced in any reaction is termed as its "standard reduction…

Q: 1. For an electrochemical copper reduction reaction at 25°C and 101 kPa, calculate (a) the Gibbs…

A: The electrochemical cell is composed of cathode and anode. The reaction at cathode of the cell is…

Q: Determine the time required to deposit 5.25 g of silver on a surfacefrom a silver nitrate solution…

Q: This is electrochemistry. Use the Nernst equation to find log Cu^2+ of each voltage.

A: When [Cu2+] = 0.050 M ,log [Cu2+] = -1.30 When [Cu2+] = 0.125 M , log [Cu2+] = -0.90 When [Cu2+]=…

Q: What mass of copper , in mg , can be deposited from copper (II) sulfate solution using a current of…

Q: 7. Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2 amps in an…

A: Given, If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2…

Q: The following cell was constructe SCE||KBr|AgBr(sat'd)|Ag. If the measured cell potential was V,…

A: Disclaimer: There is some discrepancy either in the data or the given options as the answer does not…

Q: Electrodes used in electrocardiography are disposable, andmany incorporate silver. The metal is…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: What current must be used to plate 1.75 moles of copper on an electrode in 6.25 minutes?

A: ∙Given:- no. of moles of copper =1.75 moles Time =6.25 minutes or 375s

Q: e7→ Sn E° = -0.14 v %3D e Cu E° = 0.34 v conditions, which species are prodi

A: In galvanic cell, Oxidation takes place at anode and reduction takes place at cathode. Reduction…

Q: 3. Molten magnesium chloride is electrolyzed in a cell that operates at 4.5V and 150000A. (a) How…

A: Given , Electrolysis if moltem magnesium chloride is being carried by a cell that operates at 4.5 V…

Q: The rate of deposition of copper (mass deposited per unit time) on the cathode depends on: a) The…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Ag+(aq) +…

A: The given cell reaction is, 2Ag+(aq) + H2(g) → 2Ag(s) + 2H+(aq) To find: The equilibrium constant?…

Q: Cytochrome, a complicated molecule that we will represent as CyFe2+, reacts with the air we breathe…

A: Given: The reduction reactions along with their reduction potential values are, O2g+4H+aq+4e-→2H2Ol…

Q: Calculate the concentration of the zinc sulfate solution using the Nernst equation. The Nernst…

Q: A concentration cell similar to the one shown is composed of two Ni electrodes and solutions of…

A: In concentration cell same electrode and same substance is used in solution.The only difference is…

Q: A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of…

A: The cell potential can be calculated using Nernst equation, Ecell = E° - 0.0592n log QSince, the…

Q: Calculate the cell potential in volts for following cell. Eo = +1.93 V Mg|Mg2+, 1.00 x 10-3 M||Fe2+…

Q: The Fe(3) in a 0.8202g sample was determined by coulometric reduction to fe(2) at the platinum…

A: The reaction is: Fe3++e-→Fe2+ It implies that: 96485 C is required to convert 1 mol of Fe3+ to Fe2+.…

Q: What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a…

A: From Faraday's first law of electrolysis, the weight of a chemical substance(w) deposited at an…

Q: A concentration cell similar to the one shown is composed of two Mg electrodes and solutions of…

A: A electrochemical cell is used is used convert chemical energy to electrical energy it involves a…

Q: How long (in minutes) will it take to chromium plate an object of 0.160 m2 to a thickness of 1.30…

A: We have to calculate the time taken in minutes for the deposition.

Q: Explain the principle behind FRAP (ferric reducing antioxidant power) assay. What about ABTS Assay?

A: We have to tell principle behind FRAP and also about ABTS Assay.…

Q: 5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ),…

A: The molar mass Fe atom is:- 55.85g/mol

Q: Calculate the cell potential of tho following cell at 25°C. Cr(s) | C" (1.0 X 10° M) || Ni²* (1.5 M)…

A: Given data,[Cr3+]=1.0×10-3M[Ni2+]=1.5MTemperature=25oC

Q: What mass of Ni2+Ni2+ is produced in solution by passing a current of 67.0 AA for a period of 14.0…

A: Electrochemical cell

Q: 5. Iron and Cadmium are coupled together in a poorly designed component. (a) What is the likely…

A: Given: Iron and cadmium couple.

Q: 瓦,可 212 106% Q 6: Galvanic cell presented as Fe/Fe2 //Co²/Co, If reduction potential of iron = -…

Q: Using the standard reduction potentials provided below, calculate if the oxidation of tetravalent…

A: The given half-cell reactions are: PuO22++4H++2e-⇌Pu4++2H2O; EPuO22+|Pu4+o=1.000…

Q: How can a cell consisting of a hydrogen electrode and a negative reduction potential element…

A: Hydrogen electrode: 2H+(aq)+2e-→H2( g) A platinized platinum electrode is used in this redox…

Q: In an electrolysis of copper sulphate between copper electrodes the total mass of copper deposited…

A: The solution is given below -

Q: 5. Iron and Cadmium are coupled together in a poorly designed component. (a) What is the likely…

A: Interpretation: We have to provide likely reaction in the given aqueous environment.

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cr3+(aq) +…

A: The equilibrium constant can be calculated by the standard reduction potential of the cell .

Q: What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for…

Q: Given the following table of standard reduction potentials for a hypothetical element X under an…

A: Note- Dear student it is a mutipart questions, hence I solved first three questions according to…

Q: Why might the experimentally measured reduction potentials not be equal to the theoretical reduction…

A: Actual potential of a cell will normally be found less than the ideal or nominal volts. This is…

Q: Given the following electrode reactions: 2+ Co +e Co“ E'=1,92 V 3+ Co(NH,) , +e Co(NH,), E-0,06 a.…

Q: How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water 2 by…

Q: - A student wanted to plate a silver ring with a layer of gold, He passed an electric current of 10…

Question

Analytical Chemistry II

Why is carbon used as an electrode in arc and spark sources? Explain briefly

Branch of chemistry that deals with the separation, identification, and quantification of chemical compounds. Instruments such as centrifuges, microscopes, and spectrometers are commonly used in analytical chemistry. Forensic science is well-known for being reliant on analytical chemistry techniques.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution, assuming standard-state concentrations of all species except H+ ion?
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
Hydrogen gas is produced when water is electrolyzed. 2H2O(g)2H2(g)+O2(g) A balloonist wants to fill a balloon with hydrogen gas. How long must a current of 12.0 A be used in the electrolysis of water to fill the balloon to a volume of 10.00 L and a pressure of 0.924 atm at 22°C?
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.
For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?
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-.
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.