What is the value of x in order to balance th | vedclass

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

Question

(B) To balance the redox reaction,we look at the change in oxidation states:$Mn^{2+} \rightarrow MnO_2$: $Mn$ changes from $+2$ to $+4$ (oxidation,los

Vedclass · Accepted Answer

$x=2$

Vedclass · Answer

(B) To balance the redox reaction,we look at the change in oxidation states:$Mn^{2+} \rightarrow MnO_2$: $Mn$ changes from $+2$ to $+4$ (oxidation,loss of $2e^-$).$ClO_3^- \rightarrow ClO_2$: $Cl$ changes from $+5$ to $+4$ (reduction,gain of $1e^-$).To balance the electrons,we multiply the reduction half-reaction by $2$:$Mn^{2+} + 2 ClO_3^- \rightarrow MnO_2 + 2 ClO_2$.Comparing this to the given equation $Mn^{2+} + x ClO_3^- \rightarrow MnO_2 + x ClO_2$,we find $x=2$.

What is the value of $x$ in order to balance the following redox reaction?
$Mn_{(aq)}^{2+} + x ClO_{3_{(aq)}}^{-} \rightarrow MnO_{2_{(s)}} + x ClO_{2_{(aq)}}$

Similar Questions

Identify the reaction in which monobasic and dibasic acids are formed.

Number of moles of $SnCl_2$ required for the reduction of $1$ mole of $K_2Cr_2O_7$ into $Cr^{3+}$ (in acidic medium) is:

Assuming complete ionisation,same moles of which of the following compounds will require the least amount of acidified $KMnO_4$ for complete oxidation?

Which of the following is a redox reaction?
$(i) \, CdCl_2 + 2 KOH \longrightarrow Cd(OH)_2 + 2 KCl$
$(ii) \, BaCl_2 + K_2SO_4 \longrightarrow BaSO_4 + 2 KCl$
$(iii) \, CaCO_3 \longrightarrow CaO + CO_2$
$(iv) \, 2 Ca + O_2 \longrightarrow 2 CaO$

How many moles of $K_2Cr_2O_7$ will be reduced by $1$ mole of $Sn^{2+}$ ions?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

What is the value of $x$ in order to balance the following redox reaction?$Mn_{(aq)}^{2+} + x ClO_{3_{(aq)}}^{-} \rightarrow MnO_{2_{(s)}} + x ClO_{2_{(aq)}}$