Question

In: Chemistry

For a particular redox reaction NO is oxidized to NO3– and Ag^+ is reduced to Ag....

For a particular redox reaction NO is oxidized to NO3– and Ag^+ is reduced to Ag. Complete and balance the equation for this reaction in basic solution. Phases are optional.

Solutions

Expert Solution

I balance as if acid and then add OH- to make it basic:

NO ===⇒ (NO3)^-1
1, Balance all atoms except O and H.
2. Balance the O by adding H2O
2H2O + NO =⇒ (NO3)^-

3. Balance the H by adding H+
2H2O + NO =⇒ (NO3)^- + 4H+

4. Add electrons(e-) to make the charge on both sides the same. The charge on the left is zero, and the charge on the right is +4 and -1, which gives a +3. So one adds 3e- to the right side.
2H2O + NO =⇒ (NO3)^- + 4H+ + 3e-
5. For basic soln. add add 4OH- to both sides.
4OH- + 2H2O + NO =⇒ (NO3)^- + 4H+ + 3e- + 4OH-
The H+ and OH- combines to form H2O

4OH- + 2H2O + NO =⇒ (NO3)^- + 3e- + 4H2O
Simplify by removing 2 H2O from both sides:

4OH- + NO =⇒ (NO3)^- + 3e- + 2H2O

Ag+ ==⇒ Ag
Balance the charge by adding 1e- to the left:
Ag+ + e- =⇒ Ag
4OH- + NO =⇒ (NO3)^- + 3e- + 2H2O
Multiply the Ag+ equation by 3 so the number of electrons gained equals the number lost and then
Add the two equations without the electrons.
3Ag+ + 4OH- + NO =⇒ 3Ag + (NO3)^- + 2H2O


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