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Balancing using the half reaction method in an acid

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Balance using the half reaction method in an acidic solution:
Cr(NCS)6<4->(aq) + Ce<4+> (aq) = Cr<3+>(aq) + Ce<3+> (aq) + NO3<->(aq) + CO2 (g) + SO4<2->(aq)

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Solution Summary

This solution is provided in 175 words in an attached .doc file. It demonstrates step-by-step how to balance equations and put it in half reaction form.

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Oxidation and Reduction

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2. Determine the oxidation numbers of the underlined elements in the following formulas:
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d) MnO42-

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a) SO32- + MnO4- + H+ &#8592;&#8594; Mn2+ + SO42- + H2O(l)
b) Cl2(g) + OH- &#8592;&#8594; Cl- + ClO3- + H2O(l)
c) SO42- + I- + H+ &#8592;&#8594; S2- + I2(s) + H2O(l)

4. Observations
i) A reacts spontaneously with 1 mol/L BNO3, 1 mol/L D(NO3)2 and dilute sulfuric acid. A does not react with 1 mol/L C(NO3)2.
ii) B does not react spontaneously with any of the 1 mol/L solutions above or with dilute sulfuric acid.
iii) C reacts spontaneously with dilute sulfuric acid and with 1 mol/L solutions of all the other metallic salts.
iv) D reacts spontaneously with 1 mol/L BNO3. It does not react with dilute sulfuric acid.

a) Use the observations and arrange the following five reduction half-cell reactions in order, the one with the largest positive reduction potential listed first.
A2+ + 2e- &#8594; A(s)
B+ + e- &#8594; B(s)
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D2+ + 2e- &#8594; D(s)
2H+ + 2e- &#8594; H2(g)
b) Which metal is the best reducing agent?
c) Which ion is the best oxidizing agent?

5. Calculate the voltage of a standard cell with the following half-cell reactions:
Ni(s) &#8594; Ni2+ + 2e-
2e- + Cl2(g) &#8594; 2Cl-

6. a) What metal might you fasten to the hull of an aluminum boat to give it cathodic protection in sea water?
b) Name two metals you would not use. Explain the choices.

7. By the electrolysis of water, 11.2 L of oxygen at STP was prepared.
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b) If a current of 0.5 A was used, how long did it take?

8. Aluminum is one of the most widely used metals. Aluminum is made by electrolyzing aluminum oxide in a solvent called cryolite.
a)Identify the products of the anode and cathode half-reactions that occur during the electrolysis of aluminum oxide.
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