- #1
computerex
- 68
- 0
Hello guys. I have been a lurker at these forums for quite a while now, they are very helpful if you have run into a snag in your homework. :)
What I have here is a redox reaction, and I will be very grateful if someone could confirm my answers.
H+
Equation: Ag + (NO3-) -> (Ag+) + NO
Substance reduced : Nitrate
Substance oxidized : Silver
Half reaction for oxidation : Ag - > (Ag+) + (e-)
Half reaction for reduction: NO3- + (4H+) + (e-) -> 2H2O + NO
Net balanced equation : (NO3-) + (4H+) + Ag -> 2H2O + NO + (Ag+)
Reduced equation : (NO3-) + (4H+) + Ag -> 2H2O + NO + (Ag+)
I am particularly unsure of the net balanced equation. I know I am supposed to cancel out spectator ions, but I don't think any exist within this particular reaction. Please excuse any of my blunders, I am terrible at Chemistry. :(
Edit: Is there a way to remove forum formatting ? I had everything lined up neatly...
What I have here is a redox reaction, and I will be very grateful if someone could confirm my answers.
H+
Equation: Ag + (NO3-) -> (Ag+) + NO
Substance reduced : Nitrate
Substance oxidized : Silver
Half reaction for oxidation : Ag - > (Ag+) + (e-)
Half reaction for reduction: NO3- + (4H+) + (e-) -> 2H2O + NO
Net balanced equation : (NO3-) + (4H+) + Ag -> 2H2O + NO + (Ag+)
Reduced equation : (NO3-) + (4H+) + Ag -> 2H2O + NO + (Ag+)
I am particularly unsure of the net balanced equation. I know I am supposed to cancel out spectator ions, but I don't think any exist within this particular reaction. Please excuse any of my blunders, I am terrible at Chemistry. :(
Edit: Is there a way to remove forum formatting ? I had everything lined up neatly...