Answered: 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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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
O ELECTROCHEMISTRY Designing a galvanic cell from tw... A chemist designs a galvanic cell that uses these two half-reactions: standard reduction half-reaction 2H₂O(1)+2e Write a balanced equation for the half-reaction that happens at the anode. Ered= Br₂(1)+2e Ered = +1.065 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the overall reaction. that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 significant digits. 0 0 0 O Yes O No H₂(g) + 2OH(aq) 2 Br (aq) V potential = -0.83 V - 3 ⠀ ローロ X 2 5 x10 S
2. For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M)
A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
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
Cr(s) Cr(NO3)3 A Voltaic Cell NaCl(aq) Pb(s) Pb(NO3)2 Cr³+ (aq) + 3 eCr (s) E° = -0.41 V Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb2+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. O Placing some Cr(s) in a solution containing Cr³+ ions. O Placing some Pb(s) in a solution containing Pb³+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?
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
What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cr(s)|Cr³*(0.25 M) || |2(s)|1-(0.20 M)|Pt(s)
Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? 0 0 0 0 0 0
The compound is Hg2Br2. Half reaction: Overall Voltage: Cell diagram: Calculation of Ksp:
As with any voltaic cell, the potential of zinc-copper cell changes during cell operation because the concentrations of the components do.If E°cell = + 2.71 V, [Mg2+] = 1.0 x 10-4 M and [Cu2+] = 2.0 M; find Ecell.Is the reaction at equilibrium?
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.

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