The reaction quotient (Q) for the reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right) + 3{\mathrm{H}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is given by 

$\mathrm{Q}=\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$ The reaction will proceed towards the right side, if    

1. Q>K_c

2. Q=0

3. Q=K_c

4. Q<K_c

The value of equilibrium constant of the reaction,$\mathrm{HI}\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }\frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right) + \frac{1}{2}{\mathrm{I}}_2\left(\mathrm{g}\right) \mathrm{is} 8.0.$

The equilibrium constant of the reaction, ${\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)}$ wiill be [2008]

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 $\rightleftharpoons$3C at 25$°$ 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

$\mathrm{X}\rightleftharpoons \mathrm{Y} + \mathrm{Z} ........\left(\mathrm{i}\right)$
$\mathrm{and} \mathrm{A}\rightleftharpoons 2\mathrm{B} .........\left(\mathrm{ii}\right)$

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

The relation for calculating pH of a solution containing weak acid and its salt is:

1. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

2. pH = pK_a - log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Acid}\right]}$

3. pH = pK_a + log$\frac{[\mathrm{Conjugate} \mathrm{Base}]}{\left[\mathrm{Salt}\right]}$

4. pOH = pK_a - log$\frac{\left[\mathrm{Acid}\right]}{[\mathrm{Conjugate} \mathrm{Base}]}$