MCQ
Potassium dichromate acts as a strong oxidizing agent in acidic solution. During this process, the oxidation state changes from
- A$+3$ to $+1$
- ✓$+6$ to $+3$
- C$+2$ to $+1$
- D$+6$ to $+2$

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

$\mathrm{X} \rightleftharpoons \mathrm{Y} ; \mathrm{K}_1=1.0$
$\mathrm{Y} \rightleftharpoons \mathrm{Z} ; \mathrm{K}_2=2.0$
$\mathrm{Z} \rightleftharpoons \mathrm{W} ; \mathrm{K}_3=4.0$
The equilibrium constant for the reaction $\mathrm{X} \rightleftharpoons \mathrm{W}$ is
$2 NO _{( g )}+ O _{2}( g ) \rightleftarrows 2 NO _{2}( g )$
The reaction occurring as above comes to equilibrium under a total pressure of 1 atom. Analysis of the system shows that $0.6 mol$ of oxygen are present at equilibrium. The equilibrium constant for the reaction is $.........$(Nearest integer).