Q. No.The equilibrium constant for the reaction is 4 X 10-4 at 200K. In the presence of a catalyst, the equilibrium is attained 10 times faster. Therefore, the equilibrium constant in presence of the catalyst at 200K is
1. 4 X 10-3
2. 4 X 10-4
3. 4 X 10-5
4. None of these
4. None of these
For the given reaction, the degree of dissociation of B was found to be 20% at 300 K and 24% at 500K.
\(2 \mathrm{~A}(\mathrm{~s})+\mathrm{B}(\mathrm{g}) \rightleftharpoons \mathrm{C}(\mathrm{g})+2 \mathrm{D}(\mathrm{s})+\mathrm{E}(\mathrm{s})\)
The rate of backward reaction:
| 1. | Increases with increase in pressure and temperature |
| 2. | Increases with increase in pressure and decrease in temperature |
| 3. | Depends on temperature only and decreases with increase in temperature |
| 4. | Increases with increase in concentration of B and increase in the temperature |
The pH of 0.1 M solution of anilium chloride is (Ka of = 10-6)
(1) 3.5
(2) 3
(3) 4.5
(4) none of these
1L of an aqueous solution contains 0.15mole of CH3COOH (pKa = 4.8) and 0.15 mole of CH3COONa. After the addition of 0.05 mole of solid NaOH to this solution, the pH will be :
1. 4.5
2. 4.8
3. 5.1
4. 5.4
Percentage ionisation of water at certain temperature is 3.6 X 10-7%, Calculate Kw and pH of water.
1. 10-14, pH = 6.7
2. 4 X 10-14, pH=6.7
3. 2X 10-14, pH=7
4. 10-14, pH=7
A 50 ml solution of strong acid of pH = 1 is mixed with a 50 ml solution of strong acid of pH=2. The pH of the mixture will be nearly:
(log 5.5 = 0.74)
1. 0.74
2. 1.26
3. 3.76
4. 4.50
1 litre solution of pH =4 (solution of a strong acid) is added to the 7/3 litre of water. What is the pH of resulting solution. (Log 3 = 0.48)
1. 4
2. 4.48
3. 4.52
4. 5
The pH of a solution obtained by mixing 50ml of 0.4N HCl and 50ml of 0.2M NaOH is:
1. 13
2. 12
3. 1.0
4. 2.0
Kb for a monoacidic base whose 0.10 M solution has a pH of 10.48
1. 9 X 10-6
2. 9 X 10-9
3. 9 X 10-7
4. 3 X 10-7
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