What is the emf of this cell under standard conditions?Express your answer using three significant figures.A voltaic cell utilizes the following reaction and operates at 298 K3Ce* (ag) + Cr(s)→3Ce (ag) + Cr" (ag).E = 2.35 VSubmitPrevious Answersv CorrectPart BWhat is the emf of this cell when (Ce"]=2.9 M. [Ce1= 0.10 M, and [Cr+1= 1.4x10-2 M?Express your answer using two significant figures.?E =VSubmitRequest AnswerPart CWhat is the emf of the cell when [Ce*t] = 1.4x10-2 M [Ce+] = 2.0 M, and [Cr*] = 1.9 M ?Express your answer using two significant figures.E =VSubmitRequest Answer

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What is the emf of this cell under standard conditions? Express your answer using three significant figures. A voltaic cell utilizes the following reaction and operates at 298 K 3Ce** (ag) + Cr(s)-3Ce (aq) + Cr (ag). E = 2.35 V Submit Previous Answers Correct Part B What is the emf of this cell when (Ce"] = 2.9 M. [Ce"]= 0.10 M, and [Cr1 = 1.4x10-2 M? Express your answer using two significant figures. ? E = V Submit Request Answer Part C What is the emf of the cell when [Ce**] = 1.4x10-2 M.[Ce] = 2.0 M, and [Cr]= 1.9 M? Express your answer using two significant figures. E = V Submit Request Answer

What is the emf of this cell under standard conditions? Express your answer using three significant figures. A voltaic cell utilizes the following reaction and operates at 298 K 3Ce (ag) + Cr(s)-3Ce (aq) + Cr (ag). E = 2.35 V Submit Previous Answers Correct Part B What is the emf of this cell when (Ce"] = 2.9 M. [Ce"]= 0.10 M, and [Cr1 = 1.4x10-2 M? Express your answer using two significant figures. ? E = V Submit Request Answer Part C What is the emf of the cell when [Ce] = 1.4x10-2 M.[Ce] = 2.0 M, and [Cr]= 1.9 M? Express your answer using two significant figures. E = V Submit Request Answer

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 66QAP: Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C....

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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?
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
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-.
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 concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
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?
For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a cell.