1

### AIPMT 2010 Prelims

The number of atoms in 0.1 mol of a triatomic gas is (NA = 6.02 $\times$ 1023 mol$-$1)
A
6.026 $\times$ 1022
B
1.806 $\times$ 1023
C
3.600 $\times$ 1023
D
1.800 $\times$ 1022

## Explanation

No. of atoms

= NA $\times$ No. of moles $\times$ 3

= 6.023 $\times$ 1023 $\times$ 0.1 $\times$ 3

= 1.806 $\times$ 1023
2

### AIPMT 2009

10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be
A
3 mol
B
4 mol
C
1 mol
D
2 mol

## Explanation

H2 + 1/2O2 $\to$ H2O
2 g 16 g 18 g
1 mol 0.5 mol 1 mol
10 g of H2 = 5 mol and 64 g og O2 = 2 mol

$\therefore$ In this reaction, oxygen is the limiting reagent so amount of H2O produced depends on that of O2

Since 0.5 mol of O2 gives 1 mol H2O

$\therefore$ 2 mol of O2 will give 4 mol H2O
3

### AIPMT 2008

What volume of oxygen gas (O2) measuread at 0oC and 1 atm, is needed to burn completely 1 L of propane gas (C3H8) measured under the same conditions ?
A
5 L
B
10 L
C
7 L
D
6 L

## Explanation

C3H8 + 5O2 $\to$ 3CO2 + 4H2O (balanced equation)
1 vol. 5 vol. 3 vol. 4 vol.

According to the above equation 1 vol. or 1 litre of propane requires to 5 vol. or 5 litre of O2 to burn completely.
4

### AIPMT 2008

An organic compound contains carbon, hydrogen and oxygen. Its elemental analysis gave C, 38.71% and H, 9.67%. The empirical formula of the compound would be
A
CHO
B
CH4O
C
CH3O
D
CH2O

## Explanation

Element % Atomic mass mole ratio simple ratio
C 38.71 12 ${{38.71} \over {12}} = 3.22$ ${{3.22} \over {3.22}} = 1$
H 9.67 1 ${{9.67} \over 1} = 9.67$ ${{9.67} \over {3.22}} = 1$
O 51.62 16 ${{51.62} \over {16}} = 3.22$ ${{3.22} \over {3.22}} = 1$

Hence empirical formula of the compound would be CH3O