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Question 7 1 pts title = q7a2 Use data from the table below to determine the...
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq) 1.36 O2(g)+4H+(aq)+4e? ?2H2O(l) 1.23 Br2(l)+2e? ?2Br?(aq) 1.09 NO3?(aq)+4H+(aq)+3e? ?NO(g)+2H2O(l) 0.96 Ag+(aq)+e? ?Ag(s) 0.80 I2(s)+2e? ?2I?(aq) 0.54 Cu2+(aq)+2e? ?Cu(s) 0.16 2H+(aq)+2e? ?H2(g) 0 Cr3+(aq)+3e? ?Cr(s) -0.73 2H2O(l)+2e? ?H2(g)+2OH?(aq) -0.83 Mn2+(aq)+2e? ?Mn(s) -1.18 How can the table be used to predict whether or not a metal will dissolve in HCl? In HNO3? Drag the terms on the left to the appropriate blanks on the right to...
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to be oxidised by O2 (g) in acidic aqueous solution? Select one: a. Br2 (l) b. Br- (aq) c. Ni2+ (aq) d. Ag (s) e. Cu2+ (aq) Cathode (Reduction) Half-Reaction Standard Potential E° (volts) Li+(aq) + e- -> Li(s) -3.04 K+(aq) + e- -> K(s) -2.92 Ca2+(aq) + 2e- -> Ca(s) -2.76 Na+(aq) + e- -> Na(s) -2.71 Mg2+(aq) + 2e- -> Mg(s) -2.38 Al3+(aq)...
4. (a) Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate the standard emf E° of an electrochemical cell described by the following reaction: 3 Zn + 2 Cr3+ + 2 Cr + 3 Zn? (b) What is n? (c) What is AGº for this reaction at 25°? (d) What is the equilibrium constant for this reaction at 25°? TABLE 18.1 Standard Reduction Potentials at 25°C EV) 2.87 1.61 1.51 1.36...
- 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...
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...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+ #1. In the reduction table i can see several repeated values of Fe3+ one is equal to 0.77v and the second one is equal to -0.036v so, which one do I choose? Please explain. #2.If I'm asked to find the best oxidation agent, from the values already provided (Cu+, Ag+ F2 and Fe3+) which one would it be? and how would I decide from repeated values, like in #1,...
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...
a. Cl2 b. F2 c. Br2 d. I2 e. All of the halogens have equal strength as oxidizing agents. E°(V +2.87 +1.359 +1.065 +1.23 +0.799 Table 20.1 Half Reaction F2 (8) 2e → 2F- (ag) Cl2(8) 2e → 2Cl- (aq) Br21) 2e → 2Br" (ag) 02 (elut 4H+ (ag) + 4e + 2H20 (1) Agte → Ag (5) Fe3+ (aq) → Fe2+ (aq) 12 (5) + 2e – 21 (ag) Cu2+ + 2e - Cu (s) 2H+ + 2e →...
this is the complete question (no more info) Determine the voltage (V) of the following cell at 25°C: Zn(s) | Zn2+(aq, 0.37 M) || Cl-laq, 0.75 M) C12(g, 0.750 atm)| Pt Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Hg2Cl2(s) + 2e --> 2Hg(l) + 2Cl(aq); E° = +0.27 V AgCl(s) + e --> Ag(s) + Cl (aq); E° = +0.22 V Ni2+(aq) + 2e --> Ni(s); E° =...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...