The mole fraction of the solute in a 1.00 molal aqueous solution is:
1. | 0.00177 | 2. | 0.0344 |
3. | 0.0177 | 4. | 0.1770 |
6.02x1020 molecules of urea are present in 100mL of its solution. The concentration of the solution is:
1. | 0.02M | 2. | 0.01M |
3. | 0.001M | 4. | 0.1M |
1 g of magnesium is burnt with 0.56g of oxygen in a closed vessel. The left-out reactant and its quantity are
(At. weight of Mg = 24, O=16)
1. | Mg, 0.16g | 2. | O2, 0.16g |
3. | Mg, 0.44g | 4. | O2, 0.28g |
In the Haber process, 30 L of dihydrogen and 30 L of dinitrogen were taken for the reaction, which yielded only 50% of the expected product. The composition of the gaseous mixture under the said conditions at the end is:
1. 20 L ammonia, 10 L nitrogen, 30 L hydrogen
2. 20 L ammonia, 25 L nitrogen, 15 L hydrogen
3. 20 L ammonia, 20 L nitrogen, 20 L hydrogen
4. 10 L ammonia, 25 L nitrogen, 15 L hydrogen
In the reaction, 4NH3(g)+ 5O2(g) 4NO(g) +6H2O(l)
When 1 mole of ammonia and 1 mole of O2 reacts to completion, then:
1. | 1.0 mole of H2O is produced. |
2. | 1.0 mole of NO will be produced. |
3. | All the oxygen will be consumed. |
4. | All the ammonia will be consumed. |
An element X has the following isotopic composition,
200X : 90%, 199X : 8.0%, 202X : 2.0%
The weighted average atomic mass of the naturally occurring element X is closest to:
1. | 205 u | 2. | 220 u |
3. | 196 u | 4. | 200 u |
The hydrated salt, Na2SO4.nH2O, undergoes a 55% loss in mass on heating and becomes anhydrous. The value of n will be:
1. | 5 | 2. | 3 |
3. | 7 | 4. | 10 |
The molality of a 15% (w/vol.) solution of H2SO4 of density 1.1g/cm3 is-
1. 1.2
2. 1.4
3. 1.8
4. 1.6
A partially dried clay mineral contains 8% water. The original sample contained 12% water and 45% silica. The percentage of silica in the partially dried sample is nearly:
1. | 50% | 2. | 49% |
3. | 55% | 4. | 47% |
Equal volumes of 0.1 M AgNO3 and 0.2 M NaCl are mixed. The concentration of N ions in the mixture will be:
1. | 0.1M | 2. | 0.05M |
3. | 0.2M | 4. | 0.15M |