Question

Reaction 1: I2(aq)Cu^+2(aq) Ag^+(aq)Br2(aq)

Column 1---Column 2---Column 3---Column 4---Column 5

I-(aq)---X---X---T---T
Cu(s)---T---X---T---T
Ag(s)---X---X---X---T
Br-(aq)---X---X---X---X

Reaction of metals and solution of ions

Reaction 2: Ag+(aq)Pb2+(aq)Cu2+(aq)Zn2+(aq)

Column 1---Column 2---Column 3---Column 4---Column 5

Ag(s)---X---X---X---X
Pb(s)---T---X---T---X
Cu(s)---T---X---X---X
Zn(s)---T---T---T---X

Reactions of nonmetals with solutions of ions

Column 1---Column 2---Column 3---Column 4

Br2(aq)---X---X---T
Cl2(aq)---T---X---T
I2(aq)---X---X---X

Legend: T = evidence redox reaction occured
X = no evidence of redox reaction




Hi DrBob222

Please tell me if my orderrs are correct:

Reaction 1:
Cu
I^-
Ag
Br^-

Reaction 2:
Zn
Pb
Cu
Ag

Reaction 3:
Cl2
Br2
I2

Thank you

Answer 1

hey Joseph..
i think im in ur peel class as well. I got the same results for this lab. But im only concern is he wants us to place into one table, so i would assume put all the metals together and non-metals together. What do you think? Or drbob222?

Answer 2

2 and 3 look ok to me. I'm a little confused about #1 since you have metals and non-metals mixed. Cu is correct with respect to Ag, and I^- and Br^- are placed correctly according to my chart. However, the Ag^+ + I^- reacted to give AgI (but that is not a redox reaction) and if they reacted why didn't Br^- and Ag^+? Other than that, #1 looks ok, too. One last thing you should do (and I've forgotten the original question) is to check to see how you are to order these sets. As they are ordered now, #1 and #2 are arranged with the strongest reducing agent on top and the weakest at the bottom. #3 has the strongest oxidizing agent on top and the weakest on the bottom. If that's the way they should be arranged, ok. If not you can reverse them to get what you want.

Answer 3

Of the reactions that occurred spontaneously in the individual tables, what types of qualitative changes would you observe that would indicate the reaction is proceeding?

Answer 4

change in temperature, a ppt formed, change in color.
I think the original question asked for a single table.

Answer 5

ONe more question DrBob :)

For the reactions that occurred spontaneously in the individual tables, balance these reactions assuming they are in an acidic solution.

Thanks for any further assistance we appreciate it

Answer 6

No reactions posted.

Answer 7

Reaction 1
I 2(aq) Cu2 + (aq) Ag + (aq) Br2 (aq)

Reaction 2
Ag + (aq) Pb2 + (aq) Cu2 + (aq) Zn2 +(aq)

Reaction 3
Br - (aq) Cl - (aq) I - (aq)

Answer 8

2 and 3 look ok to me. I'm a little confused about #1 since you have metals and non-metals mixed. Cu is correct with respect to Ag, and I^- and Br^- are placed correctly according to my chart. However, the Ag^+ + I^- reacted to give AgI (but that is not a redox reaction) and if they reacted why didn't Br^- and Ag^+? Other than that, #1 looks ok, too. One last thing you should do (and I've forgotten the original question) is to check to see how you are to order these sets. As they are ordered now, #1 and #2 are arranged with the strongest reducing agent on top and the weakest at the bottom. #3 has the strongest oxidizing agent on top and the weakest on the bottom. If that's the way they should be arranged, ok. If not you can reverse them to get what you want.

Answer 9

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