(A)Write 2 half cell reactions. Balance the re-dox equations in acid or base medium and calculate the standard cell pote

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A Write 2 Half Cell Reactions Balance The Re Dox Equations In Acid Or Base Medium And Calculate The Standard Cell Pote 1 (70.22 KiB) Viewed 13 times

A Write 2 Half Cell Reactions Balance The Re Dox Equations In Acid Or Base Medium And Calculate The Standard Cell Pote 2 (91.65 KiB) Viewed 13 times

(A)Write 2 half cell reactions. Balance the re-dox equations in acid or base medium and calculate the standard cell potentials of the cells formed. Show all the calculation set-ups. Assume ions are (aq), even when aq is not shown (B) Use Standard reduction potential to calculate the standard cell potential and predict if the reaction is spontaneous. (Refer to instruction at the end of this assignment) 1. MnO; + Sn? → Mn- + Sn4+ H 2. Cr20-2. + Fe(s) → Fe3+ + Cr3+ H 3. Cr3+ + NO; → Cr,0-2- + NO, H 4. MnO; + SO2 → SO2 + Mn + H* 5. Mn2+ + Bio; → Bi+ + MnO4 H* 6. IO; + CH → CIO; + 12 H 7. Cr,02 + C,H,OH → Cr3+ + CH3COH H 8. NO; + C202 → CO2 + N204 H* 9. SO32- + Cu(OH)2(S) → SO2 + Cu(OH) OH 10. BH4 + Clo; → HBO3 + Cl ОН 11. Al(OH)3() + Cr(OH)4 Al(s) + Cro2 OH 12. S,032 + CIO → 5,062- + CH OH 13. CrO2 + CIO + CI+ Cro - OH 14. MnO4 + H2C2O4 → CO2 + MnO2 OH 15. Croj + HO; → Cro2- ОН: 16. CrCl3 + H2O2(aq) → Cr 0,2 + Cl2 H

Steps for balancing a redox equation in an acidic or a basic solution 1. Find the oxidation numbers of the key elements. Draw a line from reactants to products, show the change in oxidation# of the de key element. 2. Separate into 2 half-reactions. One shows oxidation and the other shows reduction. Add electrons to the half reactions according to the change in the oxidation #, i.e., for the reduction half reaction, add to the reactant side he same number of electrons as the decrease in oxidation number, and for the oxidation half reaction add to the product side the same number of e's corresponding to the increase in oxidation number. 3. While doing step 2, make sure the key elements are balanced in each half equations and adjustment(s) accordingly. 4. Balance the half equations for oxygen: (a) In acidic solution * Add 2H* to the O-rich side for each extra oxygen. * Add H₂O to the other side for each extra oxygen. (b) In basic solution * Add H₂O to the O-rich side for extra oxygen. * Add 20H* to the O-deficient side for each extra oxygen 5. Multiply each half reaction by an appropriate factor so that the e's can Be canceled. 6. Add the 2 half reactions - # of e's in the half reactions can be canceled.

Steps for balancing a redox equation in an acidic or a basic solution 1. Find the oxidation numbers of the key elements. Draw a line from reactants to products, show the change in oxidation# of the de key element. 2. Separate into 2 half-reactions. One shows oxidation and the other shows reduction. Add electrons to the half reactions according to the change in the oxidation #, i.e., for the reduction half reaction, add to the reactant side he same number of electrons as the decrease in oxidation number, and for the oxidation half reaction add to the product side the same number of e's corresponding to the increase in oxidation number. 3. While doing step 2, make sure the key elements are balanced in each half equations and adjustment(s) accordingly. 4. Balance the half equations for oxygen: (a) In acidic solution * Add 2H* to the O-rich side for each extra oxygen. * Add H₂O to the other side for each extra oxygen. (b) In basic solution * Add H₂O to the O-rich side for extra oxygen. * Add 20H* to the O-deficient side for each extra oxygen 5. Multiply each half reaction by an appropriate factor so that the e's can Be canceled. 6. Add the 2 half reactions - # of e's in the half reactions can be canceled.