1. Questions

chem. stuff+5

9. The reaction 2 H2O(l)>>>O2(g) + 2 H2(g) requires 2.06 V, but the reaction
2 H2O(l) + 2 Cl –(aq)>>> H2(g) + 2 OH –(aq) + Cl2(g) requires 2.19 V. If a 1.0 mol/L solution of aqueous NaCl is electrolyzed, what voltage should be applied to get O2(g), but not Cl2(g)?

How would I do this?

10. The electrolysis of aqueous NaCl produces the reaction that follows.

2 H2O(l) + 2 Cl –(aq)>>> H2(g) + 2 OH –(aq) + Cl2(g)

Which other aqueous solution could be electrolyzed to produce the same reaction?

How would I do this?

12. A student wanted to produce lithium using the reaction 2 Li +(l) + 2 Cl –(l)>>> 2 Li(l) + Cl2(g) at 650°C. Give three reasons why the voltages in the reduction half-reaction table in your data booklet would not help him estimate the required voltage.
My answer:
1. It does not contain Li liquid
2. Neither does it contain Cl liquid
3. The Voltages of the equations we do have do not add up to give enough power to produce lithium.

Can u check it please?

13. Why is it sometimes possible for a weaker oxidizing agent or a weaker reducing agent to be involved in an electrolytic reaction rather than the strongest agents?

How is this possible?

20. A pot is to be electroplated with 48.6 g of nickel from a Ni(NO3)2(aq) solution. The cathode compartment of an electrolytic cell can hold 2.50 L of solution. What concentration of Ni(NO3)2(aq) solution is necessary to supply the necessary nickel?

Can u help on these questions...they r the only ones I don't get...Thanks in advance!


9. The reaction 2 H2O(l)>>>O2(g) + 2 H2(g) requires 2.06 V, but the reaction
2 H2O(l) + 2 Cl –(aq)>>> H2(g) + 2 OH –(aq) + Cl2(g) requires 2.19 V. If a 1.0 mol/L solution of aqueous NaCl is electrolyzed, what voltage should be applied to get O2(g), but not Cl2(g)?

How would I do this?
Shouldn't it be above 2.06 but below 2.19?

10. The electrolysis of aqueous NaCl produces the reaction that follows.

2 H2O(l) + 2 Cl –(aq)>>> H2(g) + 2 OH –(aq) + Cl2(g)

Which other aqueous solution could be electrolyzed to produce the same reaction? What about KCl or LiCl or any chloride whose metal salt (Na, K, Li, etc) is above hydrogen in the activity series?

How would I do this?

12. A student wanted to produce lithium using the reaction 2 Li +(l) + 2 Cl –(l)>>> 2 Li(l) + Cl2(g) at 650°C. Give three reasons why the voltages in the reduction half-reaction table in your data booklet would not help him estimate the required voltage.
My answer:
1. It does not contain Li liquid
2. Neither does it contain Cl liquid
3. The Voltages of the equations we do have do not add up to give enough power to produce lithium.
I think both 1 and 2 of your answers are another way of saying that the voltages found in your booklet are those of a 1 M solution of the ion and the solid metal (in the case of Li) or gas at 1 atm pressure vs 1 M Cl^-(in the case of Cl). In molten LiCl this isn't so. Actually this is anactivity of 1 as opposed to a concentration of 1 M. I don't understand your #3 answer.
Can u check it please?

13. Why is it sometimes possible for a weaker oxidizing agent or a weaker reducing agent to be involved in an electrolytic reaction rather than the strongest agents?
Check out how the voltage changes with concentratin; i.e., the Nernst equation.
How is this possible?

20. A pot is to be electroplated with 48.6 g of nickel from a Ni(NO3)2(aq) solution. The cathode compartment of an electrolytic cell can hold 2.50 L of solution. What concentration of Ni(NO3)2(aq) solution is necessary to supply the necessary nickel?

Can't you determine how much Ni(NO3)2 must be in 2.5 L to have a minimum of 48.6 g Ni? Actually, you would need more Ni than this.
48.6 g Ni x (1 mol Ni(NO3)2/1 mol Ni) I hope this helps.

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