Question
For the reactions that occurred spontaneously in the individual tables, balance these reactions assuming they are in an acidic solution.
Reaction 1:
Cu
I^-
Ag
Br^-
Reaction 2:
Zn
Pb
Cu
Ag
Reaction 3:
Cl2
Br2
I2
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)
Reaction 1:
Cu
I^-
Ag
Br^-
Reaction 2:
Zn
Pb
Cu
Ag
Reaction 3:
Cl2
Br2
I2
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)
Answers
Your notation is still somewhat confusing to me but here is what you do for one of the reactions. The others are done the same way.
For the copper, Ag^+ reaction:
Cu ==> Cu^+2 + 2e
Ag^+ + e ==> Ag
====================
The electrons must be kept equal; therefore, multiply the first equation by 1 and the second equation by 2, then add them.
Cu + 2Ag^+ ==> Cu^+2 + 2Ag.
The others are done the same way.
For the copper, Ag^+ reaction:
Cu ==> Cu^+2 + 2e
Ag^+ + e ==> Ag
====================
The electrons must be kept equal; therefore, multiply the first equation by 1 and the second equation by 2, then add them.
Cu + 2Ag^+ ==> Cu^+2 + 2Ag.
The others are done the same way.
Related Questions
for the redox k lab there are also two questions..
drbob222 do you think you could help
Questi...
3. Which oxidation-reduction reactions are best balanced by the half-reaction method?
A.) cov...
Classify the following reactions as precipitation reactions, oxidation-reduction reactions, or acid-...
In which reaction is energy released?
Responses
no reactions
no reactions
all reactions
a...