Question

For a particular redox reaction, NO is oxidized to NO−3 and Ag+ is reduced to Ag . Complete and balance the equation for this reaction in basic solution. The phases are optional. balanced reaction: NO + Ag^{+} -> NO_{3}^{-} + Ag NO+Ag+⟶NO−3+Ag

Answer 1

Answer:

Balanced reaction: $NO(g)+4OH^{-}(aq.)+3Ag^{+}(aq.)\rightarrow NO_{3}^{-}(aq.)+3Ag(s)+2H_{2}O(l)$

Explanation:

Oxidation reaction: $NO(g)\rightarrow NO_{3}^{-}(aq.)$

Balance O and H in basic medium: $NO(g)+4OH^{-}(aq.)\rightarrow NO_{3}^{-}(aq.)+2H_{2}O(l)$

Balance charge:$NO(g)+4OH^{-}(aq.)-3e^{-}\rightarrow NO_{3}^{-}(aq.)+2H_{2}O(l)$   ................(1)

Reduction reaction : $Ag^{+}(aq.)\rightarrow Ag(s)$

Balance charge: $Ag^{+}(aq.)+e^{-}\rightarrow Ag(s)$ ...........(2)

equation (1) + $3\times$equation (2):

$NO(g)+4OH^{-}(aq.)+3Ag^{+}(aq.)\rightarrow NO_{3}^{-}(aq.)+3Ag(s)+2H_{2}O(l)$