Electrochemistry ProcedurePb(s)Pb(s)Salt bridgecontainingNANO3(aq)2.5 M Pb2+Chida5.0x 10-M Pb2+This is example of a concentration cell.Indicate where oxidation and reduction will take place.How will the system reach equilibrium?The standard electrode potential, commonly written as E°cell, of aconcentration cell is equal to?

(b) Answer- The condition of a system when neither its state of motion nor its internal energy…

Pb(s) Pb(s) Salt bridge containing NANO3(aq) 2.5 M Pb2+ 5.0x 10-M Pb2+ s example of a concentration cell. te where oxidation and reduction will take place. vill the system reach equilibrium? tandard electrode potential, commonly written as E°cell, of a entration cell is equal to?

Pb(s) Pb(s) Salt bridge containing NANO3(aq) 2.5 M Pb2+ 5.0x 10-M Pb2+ s example of a concentration cell. te where oxidation and reduction will take place. vill the system reach equilibrium? tandard electrode potential, commonly written as E°cell, of a entration cell is equal to?

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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A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M₂ SO4 and the right half cell with a 10.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 25.0 °C. left Which electrode will be positive? x10 right X Ś ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Can you break down the problem attached?
Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative
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The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =
1.Which of the following is an electrolytic cell? a.Pb(s)|Pb2+(aq)||Zn2+(aq)|Zn(s)b.Pt(s)|Fe2+(aq), Fe3+(aq)||MnO4-(aq), Mn2+(aq)|Pt(s)c.Co(s)|Co2+(aq)||Cu2+(aq)|Cu(s)d.Ni(s)|Ni2+(aq)||Cr2O72-(aq), Cr3+(aq)|Pt(s) 2. The dissolution of NH4Cl in water is an endothermic process. If the initial temperature of water is 25°C, what is the expected final temperature of the aqueous system? a.higher than 25°C b.lower than 25°C c.half of 25°C d.still 25°C3. What is the mineral formed when Cu corrodes to form a green coating on the surface? a.Cu(NO3)2 b.CuCO3 c.Cu2O d.Cu(OH)2
Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V
The following reaction is non-spontaneous as written when the components are in their standard states, the cell potential is -0.16 V. Which of the following is true? Co(s) + Fe²*(aq) 2 Co²* (aq) + Fe(s) E =-0.16 V A. the reaction is spontaneous if [Co2+/[Fe2+] > 3.91x10-6 В. the reaction is spontaneous if [Co2+]/[Fe2+] -6 C. the reaction is spontaneous if [Co2+/[Fe2*] > 2.56x105 D. the reaction is spontaneous if [Co2*]/[Fe2+] 5