The values of Kp1 and Kp2 for the reactions
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) NH3 (g) + H2S(g), the observed pressure for reaction mixture in equilibrium is 1.12 atm at 106C. The value of Kp 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 = pKa + log
2. pH = pKa - log
3. pH = pKa + log
4. pOH = pKa - log
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
The molecule that is least likely to act as a Lewis base is:
1. CO
2. \(F^{-}\)
3. AlCl3
4. PF3
The ionisation constant of ammonium hydroxide is 1.77 x 10-5 at 298 K. Hydrolysis constant of ammonium chloride is
1. 5.65 x 10-10
2. 6.50 x 10-12
3. 5.65 x 10-13
4. 5.65 x 10-12
For a given solution pH = 6.9 at 60C, where Kw=10-12. The solution is:
1. acidic
2. basic
3. neutral
4. unpredictable
The equilibrium, 2SO2 (g) + O2 (g) 2SO3 (g)
shifts forward if:
1. a catalyst is used
2. an absorbent is used to remove SO3 as soon as it is formed
3. small amounts of reactants are used
4. none of the above
The pH of blood is maintained by CO2 by and H2CO3 in the body and chemical constituents of blood. This phenomenon is called:
1. colloidal
2. buffer action
3. acidic
4. salt balance
At temperature T, a compound AB2 (g) dissociates according to the reaction 2AB22AB(g) +B2(g) with a degree of dissociation x, which is small compared with unity. The expression for Kp, in terms of x and the total pressure P , is:
1. Px3/2
2. Px2/3
3. Px3/3
4. Px2/2