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 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)

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 in 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) $\to$4NO(g) +6H₂O(l)

When 1 mole of ammonia and 1 mole of O₂  reacts to completion, then:

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: 

The hydrated salt, Na₂SO₄.nH₂O, undergoes a 55% loss in mass on heating and becomes anhydrous. The value of n will be:

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:

Equal volumes of 0.1 M AgNO₃ and 0.2 M NaCl are mixed. The concentration of N${\mathrm{O}}_3^{-}$ ions in the mixture will be: