1. | 9.50 g | 2. | 1.25 g |
3. | 1.32 g | 4. | 3.65 g |
Match List-I with List-II:
List-I | List-II | ||
(a) | 4.48 litres of O2 at STP | (i) | 0.2 moles |
(b) | 12.022 × 1022 molecules of H2O | (ii) | 12.044 × 1023 molecules |
(c) | 96 g of O2 | (iii) | 6.4 g |
(d) | 88 g of CO2 | (iv) | 67.2 litres at STP |
(a) | (b) | (c) | (d) | |
1. | (i) | (iii) | (iv) | (ii) |
2. | (iii) | (i) | (iv) | (ii) |
3. | (iv) | (i) | (ii) | (iii) |
4. | (iii) | (i) | (ii) | (iv) |
1. | 1.32 g | 2. | 1.12 g |
3. | 1.76 g | 4. | 2.64 g |
A: | Atoms of all elements are composed of two fundamental particles. |
B: | \(9.10939 \times 10^{-31} \mathrm{~kg} \text {. }\). | The mass of the electron is
C: | All the isotopes of a given element show same chemical properties. |
D: | Protons and electrons are collectively known as nucleons. |
E: | Dalton's atomic theory regarded the atom as an ultimate particle of matter. |
1. | B, C and E only | 2. | A, B and C only |
3. | C, D and E only | 4. | A and E only |
1. | 0.705 m | 2. | 1.208 m |
3. | 1.165 m | 4. | 0.858 m |
An organic compound contains 80 % (by wt.) carbon and the remaining percentage of hydrogen. The empirical formula of this compound is:
[Atomic wt. of C is 12, H is 1]
1. | CH3 | 2. | CH4 |
3. | CH | 4. | CH2 |
In the Haber process, 30 litres of dihydrogen and 30 litres of dinitrogen were taken for the reaction which yielded only 50% of the expected product. What will be the composition of a gaseous mixture under the above condition in the end:
1. | 20 litres of ammonia, 20 litres of nitrogen, 20 litres of hydrogen |
2. | 10 litres of ammonia, 25 litres nitrogen, 15 litres of hydrogen |
3. | 20 litres of ammonia, 10 litres of nitrogen, 30 litres of hydrogen |
4. | 20 litres of ammonia, 25 litres of nitrogen, 15 litres of hydrogen |
The specific volume of cylindrical virus particle is hose radius and length are 7 Å & 10Å respectively. If \(\text{mol}^{-1}\), find the molecular weight.
1. \( 15.4 \mathrm{~kg} / \mathrm{mol} \)
2. \(1.54 \times 10^4 \mathrm{~kg} / \mathrm{mol} \)
3. \( 3.08 \times 10^4 \mathrm{~kg} / \mathrm{mol}\)
4. \(3.08 \times 10^3 \mathrm{~kg} / \mathrm{mol}\)