AG° = - â F E° ćel! n FE Consider the following reaction: 3 Pb2+ + 2 Cr(s) → 3 Pb(s) + 2 Cr3+ Using the values in Table 17.2, calculate Eell for this reaction. How many electrons are transferred in this reaction? n = Calculate AG° for this reaction. Is the reaction spontaneous under standard conditions? Justify your answer. Cell Potential and Keg We can also relate Ecell to Keq by the following equation: Ecell = RT nF %3D Consider the oxidation of zinc metal by acid (H*) under standard conditions (25°C). Write a balanced equation for this reaction. Using the values in Table 17.2, calculate Eell for this reaction. How many electrons are transferred in this reaction? n = Calculate Keg for this reaction.

AG° = - â F E° ćel! n FE Consider the following reaction: 3 Pb2+ + 2 Cr(s) → 3 Pb(s) + 2 Cr3+ Using the values in Table 17.2, calculate Eell for this reaction. How many electrons are transferred in this reaction? n = Calculate AG° for this reaction. Is the reaction spontaneous under standard conditions? Justify your answer. Cell Potential and Keg We can also relate Ecell to Keq by the following equation: Ecell = RT nF %3D Consider the oxidation of zinc metal by acid (H*) under standard conditions (25°C). Write a balanced equation for this reaction. Using the values in Table 17.2, calculate Eell for this reaction. How many electrons are transferred in this reaction? n = Calculate Keg for this reaction.

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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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
3. For the reaction: Zn(s) + 2Ag+ (aq) → Zn+2(aq) 2Ag(s). a. Determine the standard cell potential. b. Is the reaction spontaneous? If yes, write the cell notation.
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;…
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.14 minutes for a current of 1.97 A to plate 0.0672 g of metal from a solution containing M2(S04)3 (Round off the final answer to TWO decimal places. Do not include the unit.) A Moving to another question will save this response. «< Question 6 of 12 »
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 certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M₂SO4 and the right half cell with a 30.0 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 35.0 °C. Which electrode will be positive? 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. left right x10 X Ś
Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś
Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=
The standard state cell potential for the reaction below is 1.030 V. Zn(s) + Hg,Cl,(s)→ ZnCl,(aq) + 2Hg(1) Calculate the standard state Gibb's energy change (in kJ) at 298K for the reaction. O -99.4 kJ O -199 kJ O 199kJ O 99.4 kJ
Consider the following cell reaction: Ni(s) + 2 H*(? M). Ni?*(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.118 volts, what is the pH of the hydrogen electrode? pH =