3. Consider the disproportionation reaction Cl2 -- Cl + C10 a) Write the balanced reaction in...
Consider the disproportionation reaction Cl2 → Cl + C10;- Write the balanced reaction in acidic solution. Write the balanced reaction in basic solution. Calculate the Eº value under standard state conditions. | Calculate the potential at pH = 3 and [C1'] = 0.05, [CIO3 ] = 0.15
A. For the following reaction at 25 °C 2 Fe2+ (aq)+ Cl2 (9) --> 2 Fe3+ (aq) + 2 C1 (aq) Write a cell diagram for this reaction In this reaction, calculate Eºcell under standard conditions Calculate AGº from the cell potential B. C. D. Calculate K from the cell potential. E. Predict the value of Ecell for this reaction in if the concentration of is 0.150 M, is 0.100 M and the concentration of Cl- is 0.010 M. Fe2+...
The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced REDUCTION half reaction. Cl2+ NO3- ClO3-+ HNO2
F. Consider the oxidation Br2 to BrO; by the reduction of C104 to CIO-in basic aqueous solution pH=14). -) Write a balanced equation for each of the half reactions and the total reaction. - Calculate the potential and AG value for the reaction at pH=14. Is the reaction favorable? -) Calculate the potential and AG value for the reaction at pH=9. Is the reaction favorable?
Write the balanced reduction half-reaction for the following overall reaction: 2 Fe(s) + 3 Cl(aq) → 2 Fe3+(aq) + 6 Cl(aq) Cl(aq) + 2 e → 2 Cl(aq) Fe(s) + 3 → Fe3+ (aq) Fe(s) + Cl2(aq) → FeCl3(aq) Cl(aq) → 2Cl(aq) + 2 e O 3 Cl(aq) + 2e → 2 Cl(aq)
The following skeletal oxidation-reduction reaction occurs under acidic conditions. Cl- + Fe2+ ClO3- + Fe Write the balanced OXIDATION half reaction. (Enter electrons as e-.) Reactants Products
Enter electrons as e The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced REDUCTION half reaction. H2SO3 + C104 – 504 +CIO; Reactants Products Submit Answer Try Another Version 2 item attempts remaining ho
please help 11. Disproportionation a. Consider the following reaction. 3Ch 5CL + Cls. Write two balanced half equations (one oxidation, one reduction) to show the changes that the chlorine species undergoes. OXIDATION: REDUCTION: b. Is this reaction a disproportionation? Justify your answer. 12. REDOX Titration calculations a. Consider the following half equations. SO32- + H2O + SO42- + 2H+ + 2e. MnO4- + 8H. + 5e- → Mna: + 4H2O Combine these two equations to obtain the overall reaction of...
eletrochemical The following skeletal oxidation-reduction reaction occurs under acidic conditions. Cut +NO3 - HNO2 + Cu2+ Write the balanced REDUCTION half reaction. (Enter electrons as e.) Reactants Products Submit Answer Try Another Version 8 item attempts remaining The following skeletal oxidation-reduction reaction occurs under acidic conditions. Cr + Cu2+ - Cu + CIO3- Write the balanced REDUCTION half reaction. (Enter electrons as e.) - Reactants Products Submit Answer Try Another Version 10 item attempts remaining Visited The following skeletal oxidation-reduction...
Al3 (aq) + Ni(s). 3. Consider the unbalanced reaction Al(s)+ Ni2 (aq) > a. write balanced cathode half reaction b. write the balanced anode half reaction C. Write the balanced overall reaction d. Calculate E。, the cell potential. Is the reaction spontaneous as written? e Calculate Eolf [AP ] = 4.00 M, [Ni2+] = 2.00 x 10-5 M.