For the redox reaction Zn + NO_3^{-} rightarr | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The half-reactions are:Oxidation: $Zn \rightarrow Zn^{+2} + 2e^{-}$ (multiplied by $4$ to balance electrons: $4Zn \rightarrow 4Zn^{+2} + 8e^{-}$)R

Vedclass · Accepted Answer

$1, 4, 10$

Vedclass · Answer

(A) The half-reactions are:Oxidation: $Zn \rightarrow Zn^{+2} + 2e^{-}$ (multiplied by $4$ to balance electrons: $4Zn \rightarrow 4Zn^{+2} + 8e^{-}$)Reduction: $NO_3^{-} + 10H^{+} + 8e^{-} \rightarrow NH_4^{+} + 3H_2O$Adding both half-reactions gives the balanced equation:$4Zn + NO_3^{-} + 10H^{+} \rightarrow 4Zn^{+2} + NH_4^{+} + 3H_2O$The coefficients of $NO_3^{-}$,$Zn$,and $H^{+}$ are $1$,$4$,and $10$ respectively.

For the redox reaction $Zn + NO_3^{-} \rightarrow Zn^{+2} + NH_4^{+}$,the coefficients of $NO_3^{-}$,$Zn$,and $H^{+}$ in the balanced equation are respectively:

Similar Questions

How many grams of $Mg$ is required to completely reduce $100 \ mL$ of $0.1 \ M$ $NO_3^{-}$ solution using the following reaction:
$NO_3^{-} + Mg \longrightarrow Mg^{2+} + NH_3$

When $H_2S$ is passed through acidified $KMnO_4,$ we get

For the ionic reaction: $XBrO_3^{-} + YCr^{+3} + ZH_2O \rightarrow pBr_2 + qHCrO_4^{-} + rH^{+}$

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$CuO + H_2 \longrightarrow Cu + H_2O$

Which of the following reactions involves oxidation-reduction?

Vedclass Test Series

Exam Paper Generator

Online Exam Module