When the Ag* concentration is 1.12 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.524V. What is the Al3+ concentration? 3Ag*(aq) + Al(s)→3Ag(s) + A*(aq) Answer: M Submit Answer Try Another Version 3 item attempts remaining

When the Ag* concentration is 1.12 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.524V. What is the Al3+ concentration? 3Ag(aq) + Al(s)→3Ag(s) + A(aq) Answer: M Submit Answer Try Another Version 3 item attempts remaining

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter22: An Introduction To Electroanalytical Chemistry

Section: Chapter Questions

Problem 22.1QAP: Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 ...

See similar textbooks

Related questions

Q: What mass of Mg is produced (in grams) when a constant current of 0.752 A is passed through an…

A: Given current (I) = 0.752 A time (t) = 14.2 hours molar mass = 24.31 g/mol electrons transfer = 2

Q: When the Cu2+ concentration is 1.02 M, the observed cell potential at 298K for an electrochemical…

A: Given: Eo (Cr3+/Cr (s)) = -0.74 V Eo (Cu2+/Cu (s)) = 0.337 VCopper act as a cathode. Chromium acts…

Q: Q3: Consider Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli-ampere…

Q: When the Ag* concentration is 8.50×10-4 M, the observed cell potential at 298K for an…

A: The Nernst equation is given as follows, The standard cell potential of the cell is first…

Q: For the given reaction in a voltaic cell, calculate the free energy, AG°, for metal electrodes (M)…

Q: Attempt 1 Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³+ (aq)…

A: we need to calculate cell potential for the given cell

Q: When the Cu2+ concentration is 2.32x10-4 M, the observed cell potential at 298K for an…

Q: When the Pb concentration is 1.14 M, the observed cell potential at 298K for an electrochemical cell…

Q: When the Pb2+ concentration is 1.21 M, the observed cell potential at 298K for an electrochemical…

Q: TUTOR Calculate the Concentrationn of a Species Usig Cell voltage When [Cu2+] = 1.26 M, the observed…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: The EMF of the cell is calculated by below,

Q: A voltaic cell is constructed with two Zn+-Zn electrodes. The two cell compartments have [Zn+]=1.9 M…

A: Since you have posted multiple questions, we'll answer the first one. If you want any other…

Q: When the Pb2+ concentration is 1.10 M, the observed cell potential at 298K for an electrochemical…

Q: When the Cu2+ concentration is 1.04 M, the observed cell potential at 298K for an electrochemical…

Q: Galvanic Cell Using Differents Salts The electrodes used in the galvanic cell are graphite and…

A: In the galvanic cell, the half-cell reaction with greater standard reduction potential will behave…

Q: What is the E° for the cell: LIL2*(aq) || T2*(aq) | T? Final answer. two decimal places; include…

A: From the given cell notation, L is oxidised and T2+ is reduced.Oxidation takes place at anode and…

Q: Exercise 20.74 - Enhanced - with Feedback MISSED THIS? Read Section 20.6 (Pages 917 -922). A voltaic…

Q: When the Hg2+ concentration is 1.30 M, the observed cell potential at 298K for an electrochemical…

Q: Ell -0.201 V for the reaction 3Pt(s)+12C1 (aq) + 2NO₁ (aq) +8H(aq) → 3PtCl(aq) + 2NO(g) + 4H₂O(1)…

A: From E°cell we can calculate individual half cell potentials.

Q: K = Answer

Q: When [Cu2+] = 1.46 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: Reactions : Cathode: Cu2+(aq) + 2e- ——> Cu (s) Anode: Mn(s) ——> Mn2+(aq) + 2e-

Q: When the Cu²+ concentration is 9.81x10-4 M, the observed cell potential at 298K for an…

A: Given, Cu2+(aq) + Mn(s) ---> Cu(s) + Mn2+(aq) Cell potential (Ecell) = 1.428 V [Cu2+] = 9.81 ×…

Q: following reaction, when the H₂ pressure is 1.97x10-3 bar, the H+ concentration is 1.22 M, and the…

Q: When the Hg2+ concentration is 1.50 M, the observed cell potential at 298K for an electrochemical…

Q: When the Ag+ concentration is 1.34 M, the observed cell potential at 298K for an electrochemical…

Q: When the Hg2+ concentration is 6.33×10-4 M, the observed cell potential at 298K for an…

A: Interpretation : Ecell = 1.520V Hg2+ = 6.33×10-4 M

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: Given is the Nerst equation in which E° is the standard cell potential while Q is reaction quotient.…

Q: TUTOR Calculate the Concentration of a Species Using Cell Voltage When [Hg2+] = 1.16 M, the observed…

A: Now according to the equation we can see that Hg is undergoing reduction by gaining electron and Mg…

Q: When the Pb2+ concentration is 1.76×10-4 M, the observed cell potential at 298K for an…

Q: An unknown metal (M) is electrolyzed. It took 48.2 seconds for a current of 1.7 A to plate 0.0433 g…

A: Given, current = 1.71 A = 1.71 coulombs/sec Time = 48.2 sec moles of e- = 1.71 x 48.2 x (1/96485)…

Q: A concentration cell is constructed using two Fe (s) electrodes each immersed in solutions of Fe, In…

Q: An electrolytic process oxidizes nickel sufide in a two-step reaction NiS:() 2NIS(s) N (aq) + 2NIS()…

A: Second laws of Faraday electrolyte - w= z.i.t

Q: cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure…

A: The question is based on concept of electrochemistry . we have been given a cell reaction. we need…

Q: When the Pb²+ concentration is 1.02 M, the observed cell potential at 298 K for an cell with the…

Q: Calculate the cell voltage under these conditions and your answer to three significant digits please…

A: Cu 2+ + 2 e- --> Cu Eo = 0.339 V Al3+ + 3e- --> Al Eo = -1.677 VEocell = Eored –…

Q: O STUDY CHECK Sketch a semi-cell for the semi reaction below, indicate if the electrode is a…

A: Electrolysis is a process in which electricity is generated from chemical reaction. At anode…

Q: When the Ag* concentration is 8.50×10-4 M, the observed cell potential at 298K for an…

Q: MISSED THIS? Watch KCV 19.6; Read Section 19.6. You can click on the Review link to access the…

Q: When the Ag+ concentration is 3.36×10-4 M, the observed cell potential at 298K for an…

A: The Nernst equation is given as :

Q: When the Cu2+ concentration is 9.50x10-4 M, the observed cell potential at 298K for an…

A: Given, [Cu2+] = 9.50 x 10-4 M Non-standard cell potential = E = 0.985 M What is the concentration…

Q: When the Ag* concentration is 1.39 M, the observed cell potential at 298K for an electrochemical…

Q: Hi! Can u please help me on parts a-c. Thanks!

A: The given reaction is: In the given reaction, Zn is getting oxidised into Zn2+ and Ni2+ is getting…

Q: The diagram above shows the experimental setup used to electroplate a small object. A current of…

Q: equation. The standard reduction potentials listed in any reference table are only valid at the…

A: A) From the formula of standard cell potential E°cell = E°c - E°a = (-0.44) -(-2.37) = 1.93 V

Q: [References] The overall reaction and standard cell potential at 25°C for the rechargeable…

Q: When the Pb2+ concentration is 1.37 M, the observed cell potential at 298K for an electrochemical…

Q: What is the calculated value of the cell potential concentration is 1.13M, and the Ag* concentration…

A: From the given reaction: Oxidation Half-reaction : Reduction Half-reaction:

Q: A Cu/Cu²+ concentration cell has a voltage of 0.24 V at 25 °C. The concentration of Cu?+ in the…

A: Given: The voltage of a Cu/Cu2+ concentration cell at 25 ∘C = 0.24 V The concentration of Cu2+ at…

Q: 3 points Save Answer Consider the following reaction with vanadium and iron: 2 Fe²+ (aq) + √²+ (aq)…

A: Fe3+(aq) + e- -----> Fe2+. E° = +0.77 V V2+. + 2e- -----> V E° = -0.49 V

Q: Electrochemical cells can be used to measure ionic concentrations. A cell is set up with a pair of…

Question

When the Ag* concentration is 1.12 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.524V. What is the Al3+
concentration?
3Ag*(aq) + Al(s) 3Ag(s) + A³*(aq)
Answer:
M
Submit Answer
Try Another Version
3 item attempts remaining

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 with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

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
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Calculate the theoretical potential of each of the following cells. Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Pt|Cr3+(2.00 10-4M),Cr2+(1.50 10-3 M)||Pb2+ (5.60 0215 10-2M)|Pb (b) Hg|Hg22+(2.00 10-2 M)||H+(1.50 10-2 M),V3+ (2.00 10-2M),VO2+(3.00 10-3M)|Pt (e) Pt|Fe3+(3.00 10-2 M), Fe2+ (4.00 10-5M)||Sn2+ (3.50 10-2M), Sn4+ (5.50 10-4 M)|Pt
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
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-.
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 10-4M),Fe2+ (0.090 M)|Pt (c) AgBr(sat’d),Br- (0.037 M)|Ag
What is the voltage of a concentration cell of Cl ions where the concentrations are 1.045 and 0.085 M? What the spontaneous reaction?