Question

In a closed flask of 5 litres, 1.0 g of H₂ is heated from 300 to
600 K. Which statement is not correct?
(a) Pressure of the gas increases
(b) The rate of collision increases
(c) The number of moles of gas increases
(d) The energy of gaseous molecules increases

Answer 1

Incorrect statement is - (c) The number of moles of gas increases.

According to ideal gas law equation, PV = nRT. In this equation, pressure represented by p is directly proportional to temperature represented by t.

Since temperature is being increased in an enclosed flask, pressure will also increase according to given equation.

The relationship between temperature and kinetic energy is given by the formula - K.E = 3/2 kT where k is blotzmann constant, t is temperature and K.E is kinetic energy.

As the temperature increases, molecules will gain more energy, according to given equation. More energy will cause high speed movement of molecules and hence more collisions.

Number of moles are independent of temperature as they are given by formula - weight/Molecular weight.

Since neither weight nor molecular weight changes with temperature, hence number of moles will remain constant.

Answer 2

Incorrect statement - The number of moles of gas increases

Correct option -c

Step by step explanation:

(a)

Increase the temperature  the pressure of the gas will be increases.

(b)

The temperature rises, the rate of collision increases.

(c)

The number of mole of the gas remains unchanged.  It is independent of temperature as mass is independent of temperature.

(d)

The energy of gaseous molecules increases.  With increase in the temperature, the energy of gaseous molecules will be high.

Hence, correct option is "c".

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