A voltaic cell consists of two half-cells La/La3+ and Sn/Sn2+. The concentration ofSn2+ is 8.00 M. The observed voltage for the cell is 2.293 V at 25°C.What is the molar concentration of La3+ in the cell?Sn2+(aq) +2e-Sn(s)E°--0.14VLa 3+(aq) +3e- a(s) E°--2.38V(Do not enter units, use 3 significant figures in the answer. Do not use scientific notation)Your Answer:

Step 1: Step 2: Step 3: Step 4:

Answered: A voltaic cell consists of two…

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...

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What is the potential of the reaction?
Find the FALSE statement about the voltaic cell based on the two reduction half- reactions shown below. The concentrations of the ions are [Al3+] = 0.01 M, [Mn2*] = 0.1 M. A13+(aq) + 3e¯ - Al(s) E°red = -1.66 V Mn2+(aq) + 2e - Mn(s) E°red = -1.18 V Al(s) is a stronger reducing agent than Mn(s) The observed cell potential is 0.49V For the balanced equation, n = 6 and Q = [AI³+]/ [Mn2+]. Using base 10, logQ = -1. The shorthand diagram for this cell is Al(s) | AI3*(aq) || Mn²*(aq) | Mn(s).
A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode compartment, diluting the solution. O The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. No change in cell emf occurs. (b) The size of the chromium electrode is increased. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. O No change in cell emf occurs. x (c) A solution of 1.0 M CrCl3 is added to the anode compartment. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf…
A concentration cell consists of two Sn/Sn2+ half-cells. The electrolyte in compartment A is 0.13M Sn(NO3)2. The elec-trolyte in B is 0.87 MSn(NO3)2. Which half-cell houses thecathode? What is the voltage of the cell?
which reaction could be used to generate electricity in a voltaic electochemical cell at the standard conditton ? a) Pb2+(aq) + Mg(s) --> Pb(s) +Mg2+(aq) b) Zn2+(aq) + Sn(s) --> Zn(s) + Sn2+ (aq) c) NaCl(aq) + AgNO3(s) --> AgCl(s) + NaNO3(aq) d) Cu2+(aq) +4NH3(aq) --> Cu(NH3)4^2+(aq) e) none of the above please explain
Predict the potential for the following voltaic cell at 25 C:Cu(s)|CuSO4(1.29 M)||AgNO3(0.7 M)|Ag(s)
8
What would be produced by an electrolytic cell involving the following half-reactions: Pb2+(aq) + 2e- → Pb(s) E° = -0.13 V2H+(aq) + 2e- → H2(g) E° = 0.00 V a)Pb2+(aq) and H+(aq) b)Pb2+(aq) only c)Pb2+(aq) and H2(g) d)Pb(s) only e)Pb(s) and H+(aq) f)H+(aq) only g)Pb(s) and H2(g)
Consider a voltaic cell with the cell notation shown below. Which of the following statements is INCORRECT? C(s) | V³+ (aq) (1 M), VO²+ (aq) (1 M), H* (aq) (1 M) || Cr₂O7²- (aq) (4 M), Cr³+ (aq) (0.5 M), H* (aq) (1 M) | C(s) Given: VO²+ (aq) + 2 H+ *(aq) + e² = √³+ (aq) + H₂O(1) E° = +0.34 V Cr₂O7²- (aq) + 14 H* (aq) + 6 e¯ 2 Cr³+ (aq) + 7 H₂0 (1) E° = +1.33 V T = 298.15 K; R = 8.3145 J/mol-K; F = 96485 J/V-mol e The maximum work that can be generated by the cell is - 520 kJ. O Six moles of electrons are involved in the redox reaction. The equilibrium constant for the standard electrochemical reaction is e²31. O The cell potential (Ecell) is 1.00 V.
3) Use half cell potentials to determine if each reaction occur spontaneous in the direction written (yes/no). a) Ca¹2(aq) + Zn(s) - Ca(s) + Zn¹²(aq) b) Au*³(aq) + Ag(s) - Au(s) + Ag (aq) c) Co(s) + Pb (aq) - Co²(aq) + Pb(s) d) Pb(aq) + H₂S(g) -Pb¹2(aq) + S(s) ing if each metal will dissolve in 1M HCl.
Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations. Sn(s) Sn+ (aq, 0.0155 M) Ag*(aq., 1.50 M) Ag(s) net cell equation: Sn(s) +2Ag*(aq) - Sn2+ (aq) + 2Ag(s) Calculate E and Ecell at 25 °C, using standard potentials as needed. V 0.96 %3D Ecell V Ecell 0.876 %3D Incorrect
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2+ half-cell and an H2/H+ half-cell under the following conditions: [Zn2+ ] = 0.041 M [H+ ]= 1.2 M partial pressure of H2 = 0.52 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2+ (aq) + 2e Zn(s) E° = 0.76 V 2H+ (aq) + 2e H2(g) E° = 0.00 V

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