Q. No.| 1. | \(0.6 \text{ dm}^3\) of \(\text{CO},\) \(0.8 \text{ dm}^3\) of \(\text{CO}_2\) |
| 2. | \(0.8 \text{ dm}^3\) of \(\text{CO},\) \(0.8 \text{ dm}^3\) of \(\text{CO}_2\) |
| 3. | \(0.8 \text{ dm}^3\) of \(\text{CO},\) \(0.6 \text{ dm}^3\) of \(\text{CO}_2\) |
| 4. | \(0.6 \text{ dm}^3\) of \(\text{CO},\) \(0.4 \text{ dm}^3\) of \(\text{CO}_2\) |
(Molar mass of glucose: 180 g/mol)
1. 2.25 g
2. 4.5 g
3. 0.44 g
4. 1.125 g
What is the molality of a 1 M solution of compound X having density 1.25 g mL⁻¹ and molar mass 85 g mol⁻¹?
1. 0.705 m2. 1.208 m
3. 1.165 m
4. 0.858 m
An aqueous solution of NaOH has a molarity of 2 M and a density of 1.28 g cm⁻³.
Calculate the molality of the solution:
[Given: Molecular mass of NaOH = 40 g mol-1]
| 1. | 1.20 m | 2. | 1.56 m |
| 3. | 1.67 m | 4. | 1.32 m |
Which of the following is dependent on temperature?
| 1. | Molarity | 2. | Mole fraction |
| 3. | Weight percentage | 4. | Molality |
Calculate the mole fraction of the solute in a 1.00 m aqueous solution.
| 1. | 0.177 | 2. | 0.771 |
| 3. | 0.0534 | 4. | 0.0177 |
1. 90.0 g conc. HNO3
2. 70.0 g conc. HNO3
3. 54.0 g conc. HNO3
4. 45.0 g conc. HNO3
| 1. | 0.01 M | 2. | 0.001 M |
| 3. | 0.1 M | 4. | 0.02 M |
Calculate the mole fraction of solute in a 1.00 molal aqueous solution.
1. 0.0177
2. 0.0344
3. 1.770
4. 0.1770
25.3 g of sodium carbonate, Na2CO3, is dissolved in enough water to make 250 mL of a solution. If sodium carbonate completely dissociates, the molar concentrations of sodium ion, Na+ and carbonate ion, are respectively:
(molar mass of Na2CO3 = 106g mol-1)
1. 0.955 M and 1.910 M
2. 1.910 M and 0.955 M
3. 1.90 M and 1.910 M
4. 0.477 M and 0.477 M
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