Answered: Chemistry Question

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Chemistry

Chemistry Question

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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Answer the following questions using the data in Appendix L of the textbook. a. Calculate the standard cell potential for a galvanic cell made with Ni and Ag. b. Calculate the standard cell potential for a galvanic cell made with Ni and Zn.
All of the following statements regarding electrochemical cells are true except All electrochemical cells require an applied electric current. In a voltaic cell the electrons flow from the anode to the cathode. In a voltaic cell, the half reactions are separated. The salt bridge maintains electricalcontact and charge neutrality.
Consider the voltaic cell diagrammed below: Pb (s)| Pb²+ (aq)l| H2 (g)| H* (aq) | Pt (s) a) Write the balanced chemical equation that occurs in the voltaic cell depicted in the diagram. b) If the concentration of Pb2+ in this cell is 0.035 M and the pH is 1.60, what pressure of H2 (g) would keep the cell reaction in equilibrium?
Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 V
Calculate the concentration of an unknown solution in a concentration cell. A concentration cell consisting of two hydrogen electrodes (P H2- latm), where the cathode is a standard hydrogen electrode and the anode solution has an unknown pH, has a cell voltage of 0.193 V. What is the pH in the unknown solution? Assume the temperature of the solutions is 298 K. !! pH =
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;…
MnO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify the oxidizing agent and anode. C) standard cell potential? D) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?
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
Consider a voltaic cell that can be described like so. It is set up at standard conditions. A gold electrode is in contact with Au(NO3)3 (aq) and a lead electrode in contact with Pb(NO3)2 (aq) at 25 degrees C. Write true or false next to each of the following statements regarding the voltaic cell. I. Adding H20 to the lead half-cell will increase the measured cell potential. II. A salt-bridge is used to prevent charge buildup in the half-cells. III. This will result in the production of Pb2+ ions.
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O
A student constructed a voltaic cell by combining Sn/Sn2+ and Zn/Zn2+ two half cells and measured a cell potential of 0.620 V. He then constructed a voltaic cell by combining Sn/Sn2+ and Ni/Ni2+ two half cells and measured a cell potential of 0.140 V. It is seen that the tin metal precipitated out of the solution in each above cell. Except for the reduction potential of Zn which is known as -0.763V, the reduction potentials of all the other two electrodes are unknown. a. Calculate the reduction potential of Sn2+ (aq)+ 2e- ---> Sn(s). b. Calculate the reduction potential of Ni2+(aq)+2e- ----> Ni(s) c. Write the cell reaction for the cell of Sn/Sn2+ and Zn/Zn2+