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For the reaction, 2012+ + Cl2|9) -- 20:3+ + 201", 'cell is 1.78 V. Calculate E'cell...
For the reaction, 2012+ + Cl2|9) – 2013+ + 2C1, Ecel is 178 V. Calculate Ecell for the related reaction Cr3+ + Cr +C12+ +12Cl2(g). Multiple Choice None of these 178 V 09V 0 -178 089 V
Question 3 15 pts What is the correct cell voltage for the following electrochemical cell reaction? -> Cr3+ (aq) Cr(s) + Agfaq) + A9(8) E°Cr3+/cr = (-) 0.74V , EºAg+/Ag = (+) 0.80 V (-) 0.06 V (+) 0.06 V (+) 1.54 V O(-) 1.54V
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical 3 C12(a) + 2 Fe(s) - 6 Cr(aq) + 2 Fe3+ (aq) Cl2(g) + 2 + 2 Cl(aq) Fe3+ (aq) + 36 - Fe(s) E' = +1.36 V E' = -0.04 V +1.40 V O-1.40 V 0 +4.16 V O +1.32 V O-1.32 V Submit Resvest Answer
Use the following half-reactions to write 3 spontaneous reactions, calculate E°cell for each reaction, what is the n number (number of electrons transferred). Au+ (aq) + e− → Au (s) E° = 1.69 V N2O (g) + 2H+ (aq) + 2 e− → N2 (g) + H2O (l) E° = 1.77 V Cr3+ (aq) + 3 e− → Cr (s) E° = -0.74 V Question 7 0.36 pts Use the following half-reactions to write 3 spontaneous reactions, calculate Eºcell for...
1) Balance the following reaction under acidic conditions and calculate the cell potential in (V) at 298 K generated by the cell. Report your answer to the hundredths place. Cr2O72-(aq) + I-(aq) → Cr3+(aq) + I2(s) [Cr2O72-] = 2.0 M, [H+] = 1.0 M, [I-] = 1.0 M, [Cr3+] = 1.0 × 10-5 M 2) What is the value of n for the following reaction? Enter the whole number. 3Ni+(aq) + Cr(OH)3(s) + 5OH-(aq) → 3Ni(s) + CrO42-(aq) + 4H2O(l)
A. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Sn2+(aq) + 2e-Sn(s) -0.140V Cr3+(aq) + 3e-Cr(s) -0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Cl2(g) oxidize Cr(s) to Cr3+(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank. B. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Cu2+(aq) + 2e-Cu(s) 0.337V Mn2+(aq) + 2e-Mn(s) -1.180V (1) The...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
19. Choose best answer from drop-down menu: 3 points Calculate Ecell for the reaction 2 given the Ecell of reaction 1, Reaction 1: 2 Cr2+ + Cl2(g) → 2Cr3+ + 2CH Reaction 2: Cr3+ + C + Cr2+ + 1/2 Cl2(g) Ecell = 1.78 V Ecell = ? Choose 20. Choose best answer from drop-down menu: 2 points Consider the following standard reduction potentials in acid solution: E°(V) AP+ + 3e → Als) -1.66 AgBr.) + e + Agos) +...
3. Calculate the cell potential for the voltaic cell based on the following half reactions at T = 25°C: Cr3+(aq) + 3e Cr(s) E° = -0.74 V TiO2(aq) + 2H(aq) + 1e → Ti+(aq) + H2O(1) E° = + 0.10 V Where, [Cr3+] = 1.0 x 104 M, [TiO2+] = 1.0 x 10-1M, [H+] = 1.0 M, [Ti$+] = 5.0 x 10-2 M.
K for the following reaction: 7. Use the tabulated half-cell potentials to calculate 2 Cr(s) +3 Fe (aq) 2 Cr3(aq) 3 Fe(s)