$A{s}_2{S}_3+Mn{\left(N{O}_3\right)}_2+K_{2}C{O}_3\to K_{3}As{O}_4+K_{2}Mn{O}_4+NO+K_{2}S{O}_4+C{O}_2$  In this reaction select the correct options  

$$\begin{gathered} A{s}_2{S}_3+14Mn\left(N{O}_3\right)+20K_{2}C{O}_3\to 2K_{3}As{O}_4+14K_{2}Mn{O}_4+28NO+ \\ 14K_{2}S{O}_4+20C{O}_2 \end{gathered}$$One mole $\mathrm{Mn}{\left({\mathrm{NO}}_3\right)}_2$  gain 4 electrons to change to  ${\mathrm{K}}_2{\mathrm{MnO}}_4$ and lose 6 electrons  change to No according to change in oxidation states of Mn and N respectively.