Redox Reactions...

Which of the following is an intermolecular redox reaction?

What is the oxidation number of $$Mn$$ in $$KMn{O}_{4},\  {K}_{2}Mn{O}_{4},\  MnS{O}_{4},\  Mn{O}_{2}$$ and $${Mn}_{3}{O}_{4}$$ respectively?

The oxidation state of $$A,  B,$$ and $$C$$ in a compound are $$+2,  +5$$ and $$-2$$ respectively. The compound is :

$$ S$$ in $$Na_2S_2O_3$$,  $$S_4$$,  $$S_8$$ and $$Na_2S_2O_7$$.

Two half-cells have potentials $$-0.44$$ and $$0.799$$ volt respectively. These two are coupled to make a galvanic cell. Which of the following will be true?

For the redox process,
$$Zn(s) + Cu^{2+} \rightleftharpoons Zn^{2} + Cu(s)\ E_{cell}^{\circ} = + 1.10\ V$$
which graph correctly represents $$E_{cell}$$ (Y-axis) as a function of $$\log \dfrac {[Zn^{2+}]}{[Cu^{2+}]}$$ (X-axis)?

A steady current of $$10.0$$ Amps is passed through a nickel production cell of $$15$$ minutes.
Which of the following is the correct expression for calculating the number of grams of nickel produced?
Note:
$$\bullet 1\ faraday = 96,500\ Coulombs$$
$$\bullet$$ The electroytic cell involves the following half-reaction:
$$Ni_{(aq)}^{2+} + 2e^{-} \rightarrow Ni_{(s)}$$

Consider the table of standard reduction potentials shown below.

Half-reaction	$$E^{\circ}$$
$$Cl_{2} + 2e^{-}\rightarrow 2Cl^{-}$$	$$1.36\ V$$
$$O_{2} + 4H^{+} +  4e^{-} \rightarrow 2H_{2}O$$	$$1.23\ V$$
$$2H_{2}O + 2e^{-} \rightarrow H_{2} + 2OH^{-}$$	$$-0.83\ V$$
$$Rb^{+} + e^{-} \rightarrow Rb$$	$$-2.93\ V$$

Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

Consider a galvanic cell using solid $$Cu$$ and $$Fe$$ metals with their corresponding solutions.
What is the $$E^{\circ}_{cell}$$?

Standard Potential (V)	Reduction Half-Reaction
$$2.87$$	$$F_{2}(g) + 2e^{-} \rightarrow 2F^{-}(aq)$$
$$1.51$$	$$MnO_{4}^{-}(aq) + 8H^{+}(aq) + 5e^{-}\rightarrow Mn^{2+}(aq) + 4H_{2}O(l)$$
$$1.36$$	$$Cl_{2}(aq) + 3e^{-} \rightarrow 2Cl^{-}(aq)$$
$$1.33$$	$$Cr_{2}O_{7}^{2-} (aq) + 14H^{+}(aq) + 6e^{-} \rightarrow 2Cr^{3+}(aq) + 7H_{2}O(l)$$
$$1.23$$	$$O_{2}(g) + 4H^{+}(aq) + 4e^{-}\rightarrow 2H_{2}O(l)$$
$$1.06$$	$$Br_{2}(l) + 2e^{-} \rightarrow 2Br^{-}(aq)$$
$$0.96$$	$$NO_{3}^{-}(aq) + 4H^{+}(aq) + 3e^{-}\rightarrow NO(g) + H_{2}O(l)$$
$$0.80$$	$$Ag^{+}(aq) + e^{-} \rightarrow Ag(s)$$$
$$0.77$$	$$Fe^{3+} (aq) + e^{-} \rightarrow Fe^{2+}(aq)$$
$$0.68$$	$$O_{2}(g) + 2H^{+}(aq) + 2e^{-}\rightarrow H_{2}O_{2}(aq)$$
$$0.59$$	$$MnO_{4}^{-}(aq) + 2H_{2}O(l) + 3e^{-}\rightarrow MnO_{2}(s) + 4OH^{-}(aq)$$
$$0.54$$	$$I_{2}(s) + 2e^{-}\rightarrow 2I^{-}(aq)$$
$$0.40$$	$$O_{2}(g) + 2H_{2}O(l) + 4e^{-} \rightarrow 4OH^{-}(aq)$$
$$0.34$$	$$Cu^{2+}(aq) + 2e^{-} \rightarrow Cu(s)$$
$$0$$	$$2H^{+}(aq) + 2e^{-}\rightarrow H_{2}(g)$$
$$-0.28$$	$$Ni^{2+}(aq) + 2e^{-}\rightarrow Ni(s)$$
$$-0.44$$	$$Fe^{2+}(aq) + 2e^{-}\rightarrow Fe(s)$$
$$-0.76$$	$$Zn^{2+}(aq) + 2e^{-}\rightarrow Zn(s)$$
$$-0.83$$	$$2H_{2}O(l) + 2e^{-}\rightarrow H_{2}(g) + 2OH^{-}(aq)$$
$$1.66$$	$$Al^{3+}(aq) + 3e^{-}\rightarrow Al(s)$$
$$-2.71$$	$$Na^{+}(aq) + e^{-} \rightarrow Na(s)$$
$$-3.05$$	$$Li^{+}(aq) + e^{-}\rightarrow Li(s)$$

Oxidation number of 'S' in $$Na_2S_4O_6$$ is: