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

How many moles of O₂ can be obtained by electrolysis of 90 g H₂O?

• 5.0 mol

• 0.5 mol

• 2.5 mol

• 0.25 mol

An organic compound A contains 20% C, 46.66% N and 6.66% H. It gives NH₃ gas on heating with NaOH. A can be

• CH₃CONH₂

• C₆H₅CONH₂

• NH₂CONH₂

• CH₃NHCONH₂

409.

The empirical formula of a compound is CH₂. One mole of this compound has a mass 42g. Its molecular formula is

• C₃H₆

• C₂H₆

• CH₂

• C₂H₂

Aqueous solutions of hydrogen sulphide and sulphur dioxide when mixed together, yield

• sulphur trioxide and water

• hydrogen and sulphurous acid

• sulphur and water

• hydrogen peroxide and sulphur