1 M Zn(NO3)2 1 M AGNO3 2 Ag (aq) + Zn(s) → 2 Ag(s) + Zn2+ (aq) Under standard conditions, the galvanic cell shown above has a cell potential of +1.56 V using the reaction given. The salt bridge contains KNO3, which allows K* ions and NO, ions to move in the directions indicated. If KNO, in the salt bridge is replaced with KOH, some Zn(OH),(s) precipitates in the Zn-Zn(NO,), half-cell. Which of the following best explains how the cell potential is affected as Zn(OH), (s) starts to precipitate, and why? The cell potential increases because the concentration of Zn* (ag) decreases and Q. (Zn , becomes smaller. (Ag The cell potential decreases because the concentration of Zn* (aq) decreases and Q. ,becomes smaller. Ag B The cell potential increases because K ions replace Zn** ions and the reduction of K* is more thermodynamically favored than the reduction of Zn* D The cell potential stays the same because Zn(OH), (8) is not part of the redox reaction responsible for the operation of the galvanic cell.

1 M Zn(NO3)2 1 M AGNO3 2 Ag (aq) + Zn(s) → 2 Ag(s) + Zn2+ (aq) Under standard conditions, the galvanic cell shown above has a cell potential of +1.56 V using the reaction given. The salt bridge contains KNO3, which allows K* ions and NO, ions to move in the directions indicated. If KNO, in the salt bridge is replaced with KOH, some Zn(OH),(s) precipitates in the Zn-Zn(NO,), half-cell. Which of the following best explains how the cell potential is affected as Zn(OH), (s) starts to precipitate, and why? The cell potential increases because the concentration of Zn* (ag) decreases and Q. (Zn , becomes smaller. (Ag The cell potential decreases because the concentration of Zn* (aq) decreases and Q. ,becomes smaller. Ag B The cell potential increases because K ions replace Zn** ions and the reduction of K* is more thermodynamically favored than the reduction of Zn* D The cell potential stays the same because Zn(OH), (8) is not part of the redox reaction responsible for the operation of the galvanic cell.

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

Similar questions

Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is 1.120 V at 25oC. Ni(s) | Ni2+(aq) ( ? M) || Ag+(aq) (0.84 M) | Ag(s) Ni2+(aq) + 2 e- → Ni(s) Eo = -0.257 V Ag+(aq) + e- → Ag(s) Eo = 0.800 V Your answer should have 2 significant figures.
4. A galvanic cell consisting of a magnesium electrode and a standard hydrogen electrode is constructed. The cell generates a voltage, Ecell, of 2.099 V. The standard reduction potential for the two half-cell reactions are as follows: Mg²+ (aq) + 2e → Mg (s) 2H+ (aq) + 2e → H₂ (g) -2.38 V OV (i) Determine the standard cell potential, Eºcell. (ii) Assuming a Mg²+ (aq) concentration of 1 mol dm³ and a H₂ (g) pressure of 1 atm, calculate the theoretical pH of the cell. You may use concentrations/partial pressures in place of activities.
Give a clear explanation handwritten answer..provide synthesis of given bleow reactions
What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 45°C and the operating pressure is 0.06 atm. Fe2+(aq) + 2 e− ↔ Fe(s) ; [Fe2+] = 2.25 M E0 = −0.44 V Ag+(aq) + e− ↔ Ag(s) ; [Ag+] = 1.55 × 10−4 M E0 = 0.7994 V
Given the cell reaction, Zn(s) + Cut2(a the cathode in the cell is: Cu(s) Cu +2 OPt (aq) Zn(s) +2 (aq) → Zn¹2(aq) + Cu(s) +2 Zn (aq)
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(ag) +2e-→ Cu(s) +0.34 Zn2+(ag) +2e- → Zn(s) -0.76 Write the proper cell notation (with phases and concentrations) for the galvanic cell.
Suppose a galvanic cell is established using the following cell reaction, Cu(s) + 2Ag+(0.100 M) Cu2+(0.200 M) + 2Ag(s) Each compartment of the cell contains 125 mL of solution. How long would it take at a constant current of 0.10 A for the potential to drop by 10%? By how many grams will the total mass of the two electrodes change during this time period? The change in mass of the copper electrode = g The change in mass of the silver electrode = g The total change in mass of the two electrodes =
a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc electrode immersed in ZnS saturated solution water. Sketch the galvanic cell, show the anode and cathode. Write the reactions occurring at the anode and cathode , as well as the general reaction of the galvanic element.Calculate the fem of this reaction.
What is the overall cell reaction and the standard cell potential of a galvanic cell employing the following half-reactions ? NiO 2(s) +2H 2 O+2e^ -. ---> Ni(OH) 2(s) +2OH^- (aq) E ^ 0 = 0.49V Fe(OH) 2(s) +2e^ - ----> Fe (s) +2OH^- (aq) E ^ 0 = - 0.88 V
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr³+ (aq) + 3 Ca(s) → 2Cr(s) + 3Ca²+ (aq) Suppose the cell is prepared with 6.35 M Cr3+ in one half-cell and 0.492 M Ca²+ in the other half. Calculate the cell voltage under these conditions. Ered red= -0.744 V Cr³+ (aq) + 3e → Cr(s) Ca²+ (aq) + 2e → Ca(s) Ered= -2.868 V The standard cell potential (E°) for this galvanic cell is [Select] There are [Select] galvanic cell. Under these conditions, the reaction quotient is [Select] volatage is [Select] moles of electrons transferred during to operate this VV. In order to increase the cell voltage for this cell, [Select] V. ✓and the cell >
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (pH2)= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.200 V, what is the pH of the unknown solution at 298 K?