Advertisements
Advertisements
प्रश्न
A gas is at temperature 80°C and pressure 5 × 10−10 Nm−2. What is the number of molecules per m3 if Boltzmann’s constant is 1.38 × 10−23 J K−1
Advertisements
उत्तर
Temperature of a gas (T) = 80°C + 273 = 353 K
Pressure of a gas (P) = 5 × 10−10 Nm−2
Boltzmann's constant (KB) = 1.38 × 10−23 J K−1
V = 1 m3
Number of molecules, n = `"PV"/"kT"`
= `(5 xx 10^-10 xx 1)/(1.38 xx 10^-23 xx 353)`
= `(5 xx 10^-10)/(487.14 xx 10^-23)`
= 0.01026 × 1013
n = 1.02 × 1011
APPEARS IN
संबंधित प्रश्न
Which of the following shows the correct relationship between the pressure and density of an ideal gas at constant temperature?
The following graph represents the pressure versus number density for an ideal gas at two different temperatures T1 and T2. The graph implies
What is the microscopic origin of pressure?
A perfect gas of 'N' molecules, each of mass 'm', moving with velocities 'C1', 'C2', ...... .'CN' is enclosed in a cubical vessel of volume 'V'. The pressure exerted by the gas on the walls of the vessel is ______. ('p' = density of gas)
According to the assumptions made in the kinetic theory of gases, when two molecules of a gas collide with each other, then ______.
The average force applied on the walls of a closed container depends as 'Tx', where 'T' is the temperature of an ideal gas. The value of 'x' is ______.
Derive an expression for the pressure exerted by a gas on the basis of the kinetic theory of gases.
What is an ideal gas?
Does an ideal gas exist in practice?
Temperature remaining constant, if you double the number of molecules in a box, the pressure will ______.
