Which of the following is an example of a reversible reaction?

In the reaction, N₂O₄(g) $\rightleftharpoons$ 2NO₂(g), $\mathrm{\alpha }$ is that part of N₂O₄ which dissociates. The number of moles at equilibrium will be:

1. ${\left(1-\mathrm{\alpha }\right)}^2$

2. $3\mathrm{\alpha }$

3. $\mathrm{\alpha }$

4. $1+\mathrm{\alpha }$

In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be:

HI was heated in a sealed tube at 440$°$C till the equilibrium was reached. At this point, HI was found to be 22 % decomposed. The equilibrium constant for this dissociation is :

Assertion: The equilibrium constant of a reaction changes by changing the stoichiometric coefficients of the reaction.

Reason: The reaction, $2N{O}_2\left(g\right)\underset{}{\rightleftharpoons }{N}_2{O}_4\left(g\right)$

and $N{O}_2\left(g\right)\underset{}{\rightleftharpoons }\frac{1}{2}{N}_2{O}_4\left(g\right)$ have the same equilibrium constant.

1. Both assertion & reason are true and the reason is the correct explanation of the assertion.

2. Both assertion & reason are true but the reason is not the correct explanation of the assertion.

3. Assertion is a true statement but the reason is false.

4. Both assertion and reason are false statements.

PCl₅, PCl₃, and Cl₂ are at equilibrium at 500 K in a closed container and their concentrations are 0.8×10^–3 mol L^–1 , 1.2×10^–3 mol L^–1 and 1.2×10^–3 mol L^–1, respectively.
The value of  K_c  for the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) will be:
1. 1.8 × 10³ mol L^–1
2. 1.8 × 10³
3. 1.8 × 10^–3 mol L^–1
4. 0.55 × 10⁴

For the equilibrium of the reaction,\(\mathrm{HgO}(\mathrm{~s}) \rightleftharpoons \mathrm{Hg}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_ 2(\mathrm{~g}), \mathrm{K_P}\) for the reaction at a total pressure of "P" will be:

For the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)$ $+$ ${\mathrm{O}}_2\left(\mathrm{g}\right)\leftrightharpoons 2\mathrm{NO}\left(\mathrm{g}\right)$ the equilibrium constant is K₁. The equilibrium constant is K₂ for the reaction  $2\mathrm{NO}\left(\mathrm{g}\right)$ $+$ ${\mathrm{O}}_2\left(\mathrm{g}\right)$ $\leftrightharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$ $$
The value of K for the reaction given below will be:
${\mathrm{NO}}_2\left(\mathrm{g}\right)\leftrightharpoons \frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right)$ $+{\mathrm{O}}_2\left(\mathrm{g}\right)$ $$

1.  $\frac{1}{4}$ $\left(4\right)$ ${\mathrm{K}}_1$ ${\mathrm{K}}_2$

2.  ${\left[\frac{1}{{\mathrm{K}}_1{\mathrm{K}}_2}\right]}^{1/2}$

3.  $\frac{1}{\left({\mathrm{K}}_1{\mathrm{K}}_2\right)}$

4.  $\frac{1}{\left(2{\mathrm{K}}_1{\mathrm{K}}_2\right)}$

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