3.) Given the two half reactions which take place in acidic solution below, a. Balance using the half reaction method and give the overall balanced cell reaction 21-(aq) → 12(s) + 2e- Mno4- (aq) + 8H*(aq) + 5e- → Mn2*(aq) + 4H2O(I) b. Draw the voltaic cell below. What will be used for the electrodes? Label the anode and cathode, indicate the direction of electron flow, and identify the contents of each half cell and the direction of ion flow through the salt bridge. C. Write the correct half-cell notation for this reaction.

3.) Given the two half reactions which take place in acidic solution below, a. Balance using the half reaction method and give the overall balanced cell reaction 21-(aq) → 12(s) + 2e- Mno4- (aq) + 8H(aq) + 5e- → Mn2(aq) + 4H2O(I) b. Draw the voltaic cell below. What will be used for the electrodes? Label the anode and cathode, indicate the direction of electron flow, and identify the contents of each half cell and the direction of ion flow through the salt bridge. C. Write the correct half-cell notation 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...

See similar textbooks

Similar questions

A voltaic cell consists of Cu2+*/Cu and Cd2*/Cd half- cells. Each compartment has a volume of 0.500 L with the following initial concentrations: [Cu2] = 1.250 M; [Cd²*] = 0.250 M at 25°C. What is the [Cu2"] when the voltage has dropped to 0.719 V? (E° for Cu2*/Cu = 0.340 V and E° for Cd2*/Cd D -0.400 V.) %3D DEC 189 18
A voltaic cell using Cu²+/Cu and Al³+/Al half-cells is set up at standard conditions, and each compartment has a volume of 225 mL. What is the [Al³+] after the cell has delivered 0.120 A for 64.0 hours at 25°C? (E° for Cu²+/Cu = 0.340 V and E° for AI³*/AI = -1.660 V.)
A voltaic cell is constructed from a standard Cr³+1 Cr half cell (E° red = -0.740V) and a standard Fe³+ | Fe2+ half cell (Eºred = 0.771V). (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + The cathode reaction is: + The spontaneous cell reaction is: The cell voltage is V. + + + [
We will now consider the reaction of our experiment. The two half reactions for electrolysis of water are: _-) 2H₂O(l) + 2e¯¯ →>> H₂(g) + OH¯(aq) nd C) H₂O(l) → 2H+ (aq) + 1/2O₂(g) + 2e¯ The experiment is set up such that two connected funnels contain 50 mL of 0.5 M K₂SO4 and Universal Indicator. An electrode is then placed in each funnel, and an electric current is applied (Figure 1). (+) (-)
When attempting to create a voltaic cell that will produce electrical work, if a Sn2*/ Sn**couple is used as an anode what cathodic couple would produce the most electrical work? Half-Reaction E (V Clg)+ 2e 20 (ag) Cr0, (ag) + 14H" (ag) + 6e 2C "(ag) + 7H,O) MnO,() + 4H"(ag) + 2e Mn"(ag) + 2H,O) NO, ag) + 4H'(ag) + 3e NOg) + 2HOU) Ag'ag) Fe"(ag) +e Cu"(ag) + 2e = Cu(s) AgC + So, (ag) + 4H"(ag) + 2e SO,(g) + 2H,O) Cu*(ag) +e= Cu tag) Sn" (ag) + 2e Sn"(ag) +1.36 +1.33 +1.23 +0.96 Agis) +0.80 +0.77 +0.34 +0.22 +0.20 = Agir) + CT (ag +0.15 +0.13 0.00 Ph"(ag) + 2e= Phis) Sn"(ag) + 2e Sels) 2e Ni) -0.13 -0.14 -0.25 -031 -0.40 -0.44 PhSOA) + H"(ag) + 2e P(s) + HSO, (ag) Ca"(ag) + 2e Ca(s) Fels) C"(ag) + 3e Cs) Za"(ag) + 2e Zals) -0.74 -0.76 O Cu2*/Cu* O Ni2+/Ni O Cu2+/Cu O Fe3+/Fe2+
A voltaic cell is constructed based on the following reaction: Sn2* (aq) + Pb(s) Sn (s) + Pb?+ (aq) a) If the concentration of Sn2+* in the cathode half-cell is 1.00 M and the cell generates an emf of +0.22 V, what is the concentration of Pb2* in the anode half-cell? b) If the anode half-cell contains [SO,2-] = 1.00 M in equilibrium with PbSO4 (s), what is the Ksp of PBSO4?
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)
Give the balanced cell equation and determine e for the galvanic cells based on the following half-reactions. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank) H,O2 + 2H* + 2e 2H,0 Cr2 O72 +14H + 6e" 2 C* +7H,0 e° = 1.33 V e° = 1.78 V a. V 2H* + 2e H, e =0.00 V La+ +3e - La e = -2.37 V b. V 士 |3D