The equilibrium constant Br₂ $\rightleftharpoons$2Br at 500 K and 700 K are 10^-10 and 10^-5 respectively. The reaction is:

(a) endothermic                                  (b) exothermic

(c) fast                                               (d) slow

 

1. a,b

2.c,b

3.a,d

4 c,d

Solubility of a gas in liquid increases on:

1. Addition of a catalyst

2. Increasing the pressure

3. Decreasing the pressure

4. Increasing the temperature

A solution is called saturated if:

1. ionic concentration product < solubility product

2. ionic concentration product > solubility product

3. ionic concentration product $\ge$ solubility product

4. none of the above

For reaction, ${\mathrm{PCl}}_3\left(\mathrm{g}\right) + {\mathrm{Cl}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }{\mathrm{PCl}}_5\left(\mathrm{g}\right),$

the value of K_c at 250$°\mathrm{C}$ is 26. The value of K_p at this temperature will be :

1. 0.605

2. 0.57

3. 0.83

4. 0.46

The concentration of [H⁺] and concentration of [OH^-] of a 0.1M aqueous solution of 2% ionised weak monobasic acid is                                                                    

[ionic product of water = 1x 10^-14]

1. 0.02x10^-3 M and 5x10^-11 M

2. 1x10^-3 M and 3x10^-11 M

3. 2x10^-3 M and 5x10^-12 M

4. 3x10^-2 M and 4x10^-13 M

The relation for calculating pH of a weak base is:

1. pH =pK_w -1/2 pK_b + 1/2 logc

2. pH =pK_w +1/2 pK_b - 1/2 logc

3. pH =pK_w -1/2 pK_a + 1/2 logc

4. none of the above

In a closed container of 1 dm³, 8 moles of \(AB_3\)​ gas reach equilibrium following the reaction:
\(2 \mathrm{AB}_3(g) \rightleftharpoons \mathrm{~A}_2(g)+3 \mathrm{~B}_2(g)\)
What is the equilibrium constant when 2 moles of \(A_2\) are observed at equilibrium?

1. 72 mol²L^-2                     

2. 36 mol²L^-2 

3. 3 mol²L^-2                       

4. 27 mol²L^-2  

Which is Lewis base?

1. HCl               

2. HNO₃

3. HF               

4. NH₃

For a reversible reaction, if the concentrations of the reactants are doubled, the equilibrium constant will be                                                                                       

1. one-fourth                         

2. halved

3. doubled                             

4. the same

A buffer solution is prepared in which the concentration of NH₃ is 0.3 M and the concentration of ${\mathrm{NH}}_4^{+}$ is 0.20 M. If the equilibrium constant, K_b for NH₃ equals 1.8x10^-5, what is the pH of this solution?                                                                                       

1. 9.43                             

2. 11.72

3. 8.73                               

4. 9.08