Calculate the time required for a constant current of 0.969 A to deposit 0.295 g of TI(III) as Tl(s) on a cathode. t 1.03 Incorrect S Calculate the mass of TI(I) that can be deposited as Tl₂O3(s) on an anode at a constant current of 0.969 A over the same amount of time as calculated previously.

Calculate the time required for a constant current of 0.969 A to deposit 0.295 g of TI(III) as Tl(s) on a cathode. t 1.03 Incorrect S Calculate the mass of TI(I) that can be deposited as Tl₂O3(s) on an anode at a constant current of 0.969 A over the same amount of time as calculated previously.

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

Related questions

Q: Given the half-cells: Ni/Ni2+ and Fe0 /Fe2+ a) Chose the anode and cathode. b)Calculate Eo and G…

A: Since you have posted a question with multiple sub parts, we willprovide the solution only to the…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s)+Co2+(aq)↽−−⇀…

A: Given: The concentration of Ti2+ is 0.00180 M.The concentration of Co2+ is 0.813 M.The half-cell…

Q: an acidic solution containing BiO+ is electrolyzed using a current of 0.500 A. what weight of Bi…

A: From Faradays First law of electrolysis, the amount of the substance deposited(W) at the given…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.828 M…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Pb²*(aq) +…

Q: Claculate the mass of chromium

Q: How much current is required to electroplate a metal surface with 0.432 g nickel metal from a…

Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr₂(SO4)3 for 185…

A: mass of chromium (Cr) deposited = ?Current = 10.0 ATime = 185 min = 185 × 60 s = 11100 s1 F = 96485…

Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: The voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

Q: At 25 oC a zinc-copper battery is constructed as follows: Zn|Zn2+(0.1000 M)||Cu2+(2.500 M)|Cu…

A: Using Nerst equation Ecell = Eocell - (0.0591/n ) log [ Zn2+ ]/[ Cu2+ ]

Q: At 25 oC, if the potential of a Zn–H + cell is 0.55 V at 25oC when [Zn2+] = 1.0 M and PH2 = 1.0 atm,…

A: Given Temperature = 25°C = (25 + 273.15)K = 298.15 KGiven Cell Zn-HCell reaction Zn(s) + 2H+…

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

Q: (a) Write the anode and cathode reactions and the overall reaction occurring in a lead storage…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: A redox reaction is an electron transfer process where oxidation and reduction reactions occur…

Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: he voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

Q: Calculate the concentration of Cu1+ needed to produce a galvanic cell containing Cu1+ and Cu (s)…

Q: How much time (in minutes) is required to depos

Q: A concentration cell is used to measure the molar solubility of CdCO3. A saturated solution of…

Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: Interpretation: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of…

Q: n the electrolysis of a solution containing Ni2+(aq) , metallic Ni(s) deposits on the cathode.…

Q: A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a…

A: A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a…

Q: what mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

Q: 32. What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for…

A: Given that,time, t = 244.7 min = 244.7 x 60 sec = 14682 seccurrent, i = 13.6 A F = 96485…

Q: How long will it take to plate 2.5 g of copper onto a light fixture using a solution of Cu(NO3)2 and…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni=3.0 g molar mass of Ni = 58.6934 g mol-1 Current i=113.1 A Time, t = ?

Q: Consider the following reaction: MnO4 (ag) + 5FE2+ + 8H (aq) - Mn2+ (aq) + 5FE3+ (aq) + 4H2O) (aq)…

Q: %3D Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.884…

A: In an electrochemical cell, there are two compartments, the one in which oxidation reaction takes…

Q: How much time would it take for 325 mg of copper solid (atomic molar mass = 63.546 g/mol) to be…

A: Two moles of electrons give one mole of copper atom. Number of electrons required is determined as…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…

A: Cr(s)+Fe+2 (aq )<==> Cr+2 (aq)+Fe(s) [Cr+2] = 0.876 M [Fe+2] = 0.0120 M

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

Q: 5. Followed from the previous question, it was determined that K for the reaction at 25°C between…

Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

Q: Like any piece of apparatus, an electrolytic cell operates at less than 100% efficiency. A cell…

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Given that : A student constructs an electrochemical cell with a half-cell composed of a nickel…

Q: Calculate AGexn and K for each of the following reactions. Part C The disproportionation of MnO2 (s)…

Q: 32). how long it takes to deposit 1.82 g of palladium(195.8 g/mol) if a 2.0 amp current is passed…

A: Please find the attachment

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Pb2+(aq) +…

A: Pb^2+(aq) + Sn(s) -> Pb(s) + Sn^2+(aq)

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M…

A: Given data : Cr(s) + Fe2+ (aq) ==> Cr2+(aq) + Fe(s) From table : E(Fe2+/Fe) = -0.44 V…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co2*(aq) +…

A: The half reactions taking place are Reduction : Co2+ (aq) + 2 e- ------> Co (s)…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Fe³+ (aq)…

Q: 1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The…

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

Q: A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect…

A: The voltage of a reaction in the electrochemical cell is expressed in terms of the electrode…

Question

Calculate the time required for a constant current of 0.969 A to deposit 0.295 g of T1(III) as Tl(s) on a cathode.
1.03
Incorrect
S
Calculate the mass of TI(I) that can be deposited as Tl₂ O3(s) on an anode at a constant current of 0.969 A over the same amount
of time as calculated previously.
0.003305
g

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: Given data

VIEW

Step 2: Determining the time required

VIEW

Step 3: Determining the mass of the substance deposited

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 12 images

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

A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.08 V (minus 1.08 V).
Calculate the time (minutes) required for a constant current of 0.750 A to deposit 0.270 g of cobalt (II) as cobalt (II,III) oxide [Co3O4] on the anode. Assume 100% current efficiency for both cases.
Calculate the time required for a constant current of 0.885 A to deposit 0.335 g of TI(III) as TI(s) on a cathode. Calculate the mass of TI(I) that can be deposited as TI,O, (s) on an anode at a constant current of 0.885 A over the same amount of time as calculated previously.
A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -1.09 V (minus 1.09 V).
During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on the cathode if the current is kept at 11 A?
Given the half-cells: Ni/Ni2+ and Fe0 /Fe2+ a) Chose the anode and cathode. b) Calculate Eo and Delta G and K for this reaction. c) Calculate what the new cell potential (E) would be if the concentrations were [Ni2+] =.60 M and and [Fe+2] = .025M. If you let this battery run for 2 hours at 1.3 amps, what will be the new E for this battery?
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Calculate the experimental equilibrium constant, K, for the reaction (Equation 6). Your answer should have 3 sig figs. Use your answer from question 4. Question 4 + answer: Calculate the experimental standard state free energy change, ΔGo, for the reaction: ANSWER: -1.99e5 Equation 6 Attached:
A student wanted to measure the concentration of cobalt(II) ion in an aqueous solution. For the cathode half-reaction, she used a silver electrode with a 0.51 M solution of AgNO3. For the anode half-reaction, she used a cobalt electrode dipped into the aqueous solution. If the cell gave a potential of 1.043 V at 25 °C, what was the concentration of Co2+ in the solution? Half-reaction E° (V) Ag*(aq) + e- Ag(s) +0.7996 Co2+(aq) + 2 e- -0.28 Co(s) Your Answer: Answer units
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Calculate the experimental equilibrium constant, K, for the reaction Your answer should have 3 sig figs.
This part is on electrolysis: Calculate the mass of copper deposited during the electrolysis of a CuSO4 solution if a current of 20.0 amps flows for 35.0 minutes. The molar mass of copper is approximately 63.55 g/mol.
How long does it take to deposit a coating of gold 1.00 µm thick on a disk-shaped medallion 4.00 cm in diameter and 2.00 mm thick at constant current of 87 A? The density of gold is 19.3 g/cm3 and the gold is from an Au(III) solution.
A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effect is to reverse the oxidation of iron to iron (II) by causing X to oxidize to the X ion. Calculate the voltage (in V, to two decimal places) for this reaction if it takes place under standard conditions. The standard reduction potential for X is -0.90 V (minus 0.90 V).