141.

If an organic compound has C = 40%, H = 13.3% and N = 46.67%, then the empirical formula of this compound is

• CH₄N

• C₂H₈N₂

• CH₃N

• None of these

Which of the following units of energy, represents maximum amount of energy?

• Calorie

• Joule

• Erg

• Electron volt

A compound has the empirical formula CH₂O. Its vapour density is 30. Its molecular formula is

• C₂H₄O₂

• C₂H₆O

• C₂H₆O₂

• C₂H₄O

Combustion of liquid benzene in oxygen occurs as 2C₆H₆ + 15O₂ → 12CO₂ + 6H₂O. At STP, what volume (in litre) of oxygen is required for the full combustion of 3.9 g liquid benzene?

• 11.2 L

• 22.4 L

• 8.4 L

• 7.4 L

64 g of an organic compound contains 24 g of carbon, 8 g of hydrogen and the rest oxygen. The empirical formula of the compound is

• CH₂O

• C₂H₄O

• CH₄O

• C₂H₈O

1f 20 mL of 0.4 N NaOH solution completely neutralises 40 mL of a dibasic acid, the molarity of the acid solution is

• 0.1 M

• 0.2 M

• 0.3 M

• 0.4 M

Molality of a solution is equal to

• $\frac{\mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{solute}}{\mathrm{number} \mathrm{of} \mathrm{litres} \mathrm{of} \mathrm{solution}}$

• $\frac{\mathrm{number} \mathrm{of} \mathrm{g}-\mathrm{equivalents} \mathrm{of} \mathrm{solute}}{\mathrm{number} \mathrm{of} \mathrm{litres} \mathrm{of} \mathrm{solution}}$

• $\frac{\mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{solute}}{\mathrm{number} \mathrm{of} \mathrm{kilogram} \mathrm{of} \mathrm{solvent}}$

• $\frac{\mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{a} \mathrm{component}}{\mathrm{total} \mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{all} \mathrm{components}}$

The sample with largest number of atoms is

• 1g O₂(g)

• 1g Ni(s)

• 1g B(s)

• 1g N₂(g)

An organic compound containing C, H and N gives the following on analysis : C = 40%, H = 13.33% and N = 46.67%. What would be its empirical formula?

• C₂H₇N

• C₂H₇N₂

• CH₄N

• CH₃N

The normality of 0.2M H₃PO₂ is

• 0.2 N

• 0.4 N

• 0.6 N

• 0.06 N