For the questions of Exp 20 Electrochemistry,Part B: EMF of Galvanic CellTable 2: Electromotive force of the galvanic cell found throughthe mixtures of different solutions in part B of the experimentExperiment Solution A Electrode A Solution BElectrode B#45n2+SnCu2+Cu#7Zn2+Zn0.1 M KCIAg WireAnswer the following question(s).b) Calculate E cell for Experiment #4. For the questions of Exp 20 Electrochemistry,Part B: EMF of Galvanic CellTable 2: Electromotive force of the galvanic cell found throughthe mixtures of different solutions in part B of the experimentExperiment Solution A Electrode A Solution BElectrode B#4Sn2+SnCu2+Cu#7Zn2+Zn0.1 M KCIAg WireAnswer the following question(s).c) Calculate E°cell for Experiment #7.

the equilibrium constant (Kp) for the vaporization of bromine at 59.7°C:Bromine Vaporization…

Answered: For the questions of Exp 20…

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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Draw the galvanic cell from the following half-reactions (use KCl as salt bridge) Al3 + aq + 3rd → Als Ni2 + aq + 2é → Ni (s) Indicates the anode and cathode Indicates where oxidation and reduction occur Indicates the direction of movement of electrons. Indicates the direction of movement of the ions. Write the balanced ionic equation of this equation
Consider the galvanic cell based on the following half-reactions. Ag+ + e Ni²+ + 2e →→ Ni (a) Determine the overall cell reaction and calculate Omit states-of-matter from your answer.) chemPad XX→ (c) 8 cell → Ag 8⁰ = +0.80 V 8° -0.23 V Calculate 8 Help Greek º (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. AGO kJ K (in V). (Use the lowest possible whole number coefficients. cell (in V) at 25°C when [Ag+] = 1.0x10-4 M and [Ni²+] = 1.0×10-² M. cell V
Will the potential of the galvanic cell change if we add the same amount of water to the electrolyte solutions that make up the galvanic cell?
3. Given that the whole standard potential of a Zn-Mg cell is +1.61 V and the standard reduction potential of Zn²+ → Zn is -0.76 V, what is the standard reduction potential of Mg2+→ Mg? -
A table of standard electrode potentials is necessary for many of the following question(s). Consider the following reaction: If a galvanic cell utilizes this reaction and the initial concentrations are [Hg 2 2+] = 0.10 M, [Sn 2+] = 0.30 M, and [Sn 4+] = 0.20 M, what will be E cell under these conditions? 2+ (aq) + Sn2+ (aq) → Sn4+ (aq) + 2Hg(s) Hg2 a. 0.68 V O b. 0.66 V O c. 0.61 V O d. 0.74 V O e. 0.57 V
If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how many grams of Cu will plate out onto the cathode?
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?
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
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.
Here is a drawing of an electrochemical cell: the reactions that occur in both halves of the cell are:Sn2 + (aq) + 2e- -> Sn (s) E = -0.14X3 + (aq) + 3e- --> X (s) E =?A. At the close of the circuit, electrons pass and the mass of Sn (s) increases. Mark the anode, cathode, and direction of flow of electrons in the electrical circuit.B. If the standard cell potential is 0.6 volts, what is the redox potential of the half-cell response of X + 3 / X?C. Write the balanced equation for the cell.D. Changed the Sn2 + concentrations from 1 M to 0.5M, and the concentrations of X + 3 from 1M to 0.10M calculated the cell potential in this case.

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