MCQ
What is $X$ in the following reaction?


- ✓$CH _{3} OH , H _{2} SO _{4}$
- B$CH _{3} OH , CH _{3} O ^{-} Na^+$
- C$H _{2} O _{/} H _{2} SO _{4}$ followed by $CH _{3} OH$
- D$CH _{3} MgBr _{\text {/ether }}$ followed by $H _{3} O ^{+}$


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$2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$
The degree of dissociation is $x$ and is small compared to $1.$ The expression relating the degree of dissociation $(x)$ with equilibrium constant $K_P$ and total pressure $P$ is
$SO_3(g) \rightleftharpoons SO_2(g)+ \frac{1}{2} O_2(g)$
is $K_c= 4.9 \times 10^{-2}.$ The value of $K_c$ for the reaction
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$
will be