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2. Net lonic Equations - use the directions below to write net ionic equations for the 15 possible electrode combinations. Pay special attention to Step 7 to write net ionic equations for Redox reactions. Directions For Writing Molecular, lonic, And Net lonic Equations: 1. Molecular Equation: balance the molecular equation by predicting the products and changing the coefficients so that all atoms are balanced. Equations must be balanced to obey the Law of Conservation of Matter 2. lonic Equation: the ionic equation is obtained by breaking apart into ions any strong acid, strong base or soluble salt that has an after its formula the lon's new coefficient will equal the coefficient (from the balanced equation) TIMES the lon's subscriptie 2 Na2SO, becomes 4 Na and 2 50/?) 3. Do Not Break Apart any reactant or product that has an or more after its formula - list it exactly as it appears in the molecular equation. 4. Do Not Break Apart a weak acid or base that has an after its formula - by definition a weak acid (or base) is not 100% ionized so it is represented as a molecule and not as ons 5. Net lonic Equation: write the net ionic equation by cancelling out any spectator ions (ions that appear on both sides of the equation) and simplifying the coefficients the smallest whole number ratio (if necessary) 6. Make sure to include the charge and state for the ions and molecules all molecules have a charge of zero. 7. As a final check, the total charge on the reactant side must equal the total charge on the product side - this fact will aid you in writing Redox (Reduction - Oxidation) reactions 1. Ou electrode + Fe electrode Work Problem 2. Pb electrode Fe electrode

Answer 1

1. Cu electrode + Fe electrode

Standard Electrode Potential (SRP) of Cu > Fe. So,

Cathode - Cu and Anode - Fe

Fe_(s) + Cu²⁺_(aq)→ Fe²⁺_(aq) + Cu_(s)

2. Pb electrode + Fe electrode

Standard Electrode Potential (SRP) of Pb > Fe. So,

Cathode - Pb and Anode - Fe

Fe_(s) + Pb²⁺_(aq)→ Fe²⁺_(aq) + Pb_(s)

3. Ni electrode + Fe electrode

Standard Electrode Potential (SRP) of Ni > Fe. So,

Cathode - Ni and Anode - Fe

Fe_(s) + Ni²⁺_(aq)→ Fe²⁺_(aq) + Ni_(s)

4. Sn electrode + Fe electrode

Standard Electrode Potential (SRP) of Sn > Fe. So,

Cathode - Sn and Anode - Fe

Fe_(s) + Sn²⁺_(aq)→ Fe²⁺_(aq) + Sn_(s)

5. Zn electrode + Fe electrode

Standard Electrode Potential (SRP) of Fe > Zn. So,

Cathode - Fe and Anode - Zn

Zn_(s) + Fe²⁺_(aq)→ Zn²⁺_(aq) + Fe_(s)

6. Cu electrode + Zn electrode

Standard Electrode Potential (SRP) of Cu > Zn. So,

Cathode - Cu and Anode - Zn

Zn_(s) + Cu²⁺_(aq)→ Zn²⁺_(aq) + Cu_(s)

7. Pb electrode + Zn electrode

Standard Electrode Potential (SRP) of Pb > Zn. So,

Cathode - Pb and Anode - Zn

Zn_(s) + Pb²⁺_(aq)→ Zn²⁺_(aq) + Pb_(s)

8. Ni electrode + Zn electrode

Standard Electrode Potential (SRP) of Ni > Zn. So,

Cathode - Ni and Anode - Zn

Zn_(s) + Ni²⁺_(aq)→ Zn²⁺_(aq) + Ni_(s)

9. Sn electrode + Zn electrode

Standard Electrode Potential (SRP) of Sn > Zn. So,

Cathode - Sn and Anode - Zn

Zn_(s) + Sn²⁺_(aq)→ Zn²⁺_(aq) + Sn_(s)

10. Cu electrode + Sn electrode

Standard Electrode Potential (SRP) of Cu > Sn. So,

Cathode - Cu and Anode - Sn

Sn_(s) + Cu²⁺_(aq)→ Sn²⁺_(aq) + Cu_(s)

11. Pb electrode + Sn electrode

Standard Electrode Potential (SRP) of Pb > Sn. So,

Cathode - Pb and Anode - Sn

Sn_(s) + Pb²⁺_(aq)→ Sn²⁺_(aq) + Pb_(s)

12. Ni electrode + Sn electrode

Standard Electrode Potential (SRP) of Sn > Ni. So,

Cathode - Sn and Anode - Ni

Ni_(s) + Sn²⁺_(aq)→ Ni²⁺_(aq) + Sn_(s)

13. Cu electrode + Ni electrode

Standard Electrode Potential (SRP) of Cu > Ni. So,

Cathode - Cu and Anode - Ni

Ni_(s) + Cu²⁺_(aq)→ Ni²⁺_(aq) + Cu_(s)

14. Pb electrode + Ni electrode

Standard Electrode Potential (SRP) of Pb > Ni. So,

Cathode - Pb and Anode - Ni

Ni_(s) + Pb²⁺_(aq)→ Ni²⁺_(aq) + Pb_(s)

15. Cu electrode + Pb electrode

Standard Electrode Potential (SRP) of Cu > Pb. So,

Cathode - Cu and Anode - Pb

Pb_(s) + Cu²⁺_(aq)→ Pb²⁺_(aq) + Cu_(s)