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Consider the following redox reaction 3 502 + 3 H2O + CIO3 3 8042- + 6H+...
Given the following two half-reactions, CIO3 +64 +6H+ = Clº + 3H20 HOCI + 2e +H+ = Clº + H20 E° = 1.446 V, E° = 1.481 V, what is Eº for the half-reaction representing the oxidation of HOCI to CIO,?
- cellpotentials and standard reduction potential table. -Determining the Nernst equation and finding the Faraday constant. If you can explain how to solve for each part please. 25°C Standard Reduction Potentials in Aqueous solution a 2.87 Reduction half-reaction 2F (a 1.77 2H2O 1.692 2e 2H (a Au (s 1.085 PbSO4 (s) 2H20. Au (ag) 2e 1.51 4H20 Mn 1.50 5e 8H (a Mno4 (a Au(S 1.36 3e 2Cl (aq 1.33 2e 2Cr3 (ag) 7H20 C12 6e- 1.229 14H 2H2O 1.08...
Consider the following redox reaction MnO4- + SO32- —→ SO42- + MnO2 a) Write a balanced oxidation half reaction b) Write a balanced reduction half reaction c) Which species is the oxidizing and reducing agents d) Write the overall BALANCED ionic equation UNDER BASIC CONDITIONS
3. Calculate the redox potential (in volts) for a LiMnO2/graphite battery. (Redox reaction) MnO4- + 8H + 5e- → Mn2+ (aq) + 4H2O (+1.51 V) MnO2 + 4H +2e- → Mn2+ (aq) + 2H2O (+1.22 V) xLi+ + C6 + e- → LixC5 (-3.00 V) 1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f....
4. Consider the following reactions: Table 2. 2 CIO" (aq) + 4* (aq) + 2e → A ) + 2 H20() 2 CIO3(aq) +12 H(aq) + 10 - A ) + 6H2O() Cl() +2e" 20"(aq) 2 Co (aq) + 4H+ (aq) + 4 + 2 co(aq) + 2 H20(0) 2 Clo; (aq) + 4H* (aq) + 4e-2003(aq) + 2 H20) 2 C103(aq) + 4H+ (aq) + 4e - 2 C10(aq) + 2 H2O() E .163 E=147 E=136 E 1194 E=115...
1. How do I read the half reaction table? 2. If im asked for the best reducing agent from Cu+, Ag+, F2, and Fe3+, where do I look first in the table? before the arrow or after the arrow? 3. Sometimes a value that has originally a positive (V) from the table it will have the negative sign in a homework problem, and viceversa, so the question is, how do I use the positive and negative signs in respect to...
Consider the following redox reaction. 2MnO−4(aq)+2H2O(l)+6H+(aq)2Mn2+(aq)+5H2O2(l) The standard reduction potentials for the species in the reaction are listed below: H2O2(l)+2H+(aq)+2e−2H2O(l) E°red,H2O2 = 1.776 V MnO−4(aq)+8H+(aq)+5e−Mn2+(aq)+4H2O(l) E°red, MnO4 - =1.507 Calculate E° =? V
For all of the following experiments, under standard conditions, which species could be spontaneously produced? A lead wire is placed in a solution containing Cu2+ yes no Cu yes no PbO2 yes no No reaction Crystals of I2 are added to a solution of NaCl. yes no I- yes no No reaction yes no Cl2 A silver wire is placed in a solution containing Cu2+ no yes Cu no yes No reaction no yes Ag+ Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
Question 20 (5 points) Using the following standard reduction potentials: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = +1.69 V PbO2 + 4H+ + 2e → Pb2+ + 2H20 E° = +1.46 V The standard cell voltage for the reaction PbSO4(s) Pb2+ + SO42- is V. Please enter your answer in decimal form, such as 2.5, and keep the correct number of significant figures.
Question 20 (5 points) Using the following standard reduction potentials: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = +1.69 V PbO2 + 4H+ + 2e Pb2+ + 2H20 E° = +1.46 V is The standard cell voltage for the reaction PbSO4(s) → Pb2+ + SO42- V. Please enter your answer in decimal form, such as 2.5, and keep the correct number of significant figures.