The formation of phosgene is represented as,

            CO + Cl₂ $\rightleftharpoons$COCl₂

The reaction is carried out in 500 mL flask. At equilibrium o.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl₂ are present. The equilibrium constant of the reaction is:

1. 30                     

2. 15

3. 5                       

4. 3

The reaction quotient \(\text (Q)\) for the reaction, \(\mathrm{N}_2(\mathrm{g})+3 \mathrm{H}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{g})\) is given by \(\mathrm{Q}=\dfrac{[\mathrm{NH}_3]{ }^2}{[\mathrm{N}_2 ][\mathrm{H}_2]^3}\).
At which of the following condition, the reaction will proceed towards the right side?

1. \(Q>K_c\)
2. \(Q=0\)
3. \(Q=K_c \)
4. \(Q<K_c\)

The value of equilibrium constant of the reaction,$\mathrm{HI}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\rightleftharpoons }\frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\frac{1}{2}{\mathrm{I}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>8.0.$

The equilibrium constant of the reaction, ${\mathrm{H}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{I}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)}$ wiill be:

1. $\frac{1}{16}$ 

2. $\frac{1}{64}$

3. 16

4. $\frac{1}{8}$

Which salt undergoes hydrolysis?

1. CH₃COONa                                     

2. KNO₃

3. NaCl                                               

4. K₂SO₄

The hydrolysis of the salt of a strong acid and a weak base is called:

1. Anionic hydrolysis

2. Cationic hydrolysis

3. Amphoteric hydrolysis

4. None of the above

For the reaction, A+B \(⇌ \)3C at \(​25^{\circ}C​\), a 3 litre vessel contains 1, 2, and 4 mole of A, B and C respectively. If K_c for the reaction is 10, then the reaction will proceed in:

1. forward direction                           

2. backward direction

3. in either direction                           

4. in equilibrium

Which of the following is most soluble in water?

1. MnS (K_sp = 8x10^-37)         

2. ZnS (K_sp = 7x10^-16)

3. Bi₂S₃ (K_sp = 1x10^-70)       

4. Ag₂S (K_sp = 6x10^-51)

The compound that does not act as Lewis acid is:

1. AlCl₃                                           

2. BF₃

3. NH₃                                             

4. FeCl₃

The values of K_p1 and K_p2 for the reactions

$<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\mathrm{X}\rightleftharpoons \mathrm{Y}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\mathrm{Z}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>........\left(\mathrm{i}\right)$
$\mathrm{and}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\mathrm{A}\rightleftharpoons 2\mathrm{B}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>.........\left(\mathrm{ii}\right)$

are in ratio of 9:1, if degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio 

1. 3:1

2. 1:9

3. 36:1

4. 1:1

For NH₄HS(s) $\rightleftharpoons$NH₃ (g) + H₂S(g), the observed pressure for reaction mixture in equilibrium is 1.12 atm at 106$°$C. The value of K_p for the reaction is:

1. 3.136 atm²                           

2. 0.3136 atm²

3. 31.36 atm²                           

4. 6.98 atm²