1
MCQ (Single Correct Answer)

AIPMT 2009

The energy absorbed by each molecule (A2) of a substance is 4.4 $$ \times $$ 10$$-$$19 J and bond energy per molecule is 4.0 $$ \times $$ 10$$-$$19 J. The kinetic energy of the molecule per atom will be
A
2.2 $$ \times $$ 10$$-$$19 J
B
2.0 $$ \times $$ 10$$-$$19 J
C
4.0 $$ \times $$ 10$$-$$20 J
D
2.0 $$ \times $$ 10$$-$$20 J

Explanation

Energy absorbed by each molecule = Bond energy per molecule + Kinetic energy per molecule

$$ \Rightarrow $$ 4.4 × 10–19 J = 4.0 × 10–19 J + Kinetic energy per molecule

$$ \Rightarrow $$ 0.4 × 10–19 = Kinetic energy per molecule

Kinetic energy per atom =
Kinetic energy per molecule
2


=
0.4 × 10–19
2
= 0.2 × 10–19 J

= 2 × 10–20 J
2
MCQ (Single Correct Answer)

AIPMT 2008

Volume occupied by one molecule of water (density = 1 g cm$$-$$3) is
A
3.0 $$ \times $$ 10$$-$$23 cm3
B
5.5 $$ \times $$ 10$$-$$23 cm3
C
9.0 $$ \times $$ 10$$-$$23 cm3
D
6.023 $$ \times $$ 10$$-$$23 cm3

Explanation

1 mole of water contains 6.023 × 1023 molecules of water

6.023 × 1023 molecules of water weigh = 18 g

So, 1 molecule of water weighs = $${{18} \over {6.023 \times {{10}^{23}}}}$$

Now, volume of 1 molecule of water

=
Mass of 1 molecule of water
Density of water
.

= $${{18} \over {6.023 \times {{10}^{23}}}} \times {1 \over {1\,g\,c{m^{ - 3}}}}$$

= 3 $$ \times $$ 10-23 cm3
3
MCQ (Single Correct Answer)

AIPMT 2008

If a gas expands at constant temperature, it indicates that
A
kinetic energy of molecules remains the same
B
number of the molecules of gas increases
C
kinetic energy of molecules decreases
D
pressure of the gas increases.

Explanation

Kinetic energy of a gas is expressed as

K.E = $${3 \over 2}nRT$$

Thus, on expansion of fixed amount of gas at constant temperature the kinetic energy remains constant.
4
MCQ (Single Correct Answer)

AIPMT 2002

Van der Waal's real gas, acts as an ideal gas, at which conditions?
A
High temperature, low pressure
B
Low temperature, high pressure
C
High temperature, high pressure
D
Low temperature, low pressure

Explanation

At higher temperature and low pressure real gas acts as an ideal gas.

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