MCQ
An unknown compound ‘$D’,$ first oxidised to aldehyde and then acitic acid by a dilute solution of${K_2}C{r_2}{O_7}$ and ${H_2}S{O_4}$. The unknown compound $‘D$’ is
- A$C{H_3}CHO$
- B$C{H_2}C{H_3}OH$
- ✓$C{H_3}C{H_2}OH$
- D$C{H_3}C{H_2}C{H_3}$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
$2 \mathrm{H}_{2}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
the observed rate expression is, rate $=\mathrm{k}_{\mathrm{f}}[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right] .$ The rate expression of the reverse reaction is
$S{O_2} + N{O_2} \rightleftharpoons S{O_3} + NO$
If we take one mole of each of four gases in one $L$ container. What would be equilibrium concentration of $NO$ and $NO_2$ respectively