Advertisements
Advertisements
Question
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
Solution
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
RELATED QUESTIONS
A sample of an ideal gas is at equilibrium. Which of the following quantity is zero?
Two identically sized rooms A and B are connected by an open door. If the room A is air-conditioned such that its temperature is 4°C lesser than room B, which room has more air in it?
The ratio γ = `"C"_"p"/"C"_"v"` for a gas mixture consisting of 8 g of helium and 16 g of oxygen is ____________.
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?
If 1020 oxygen molecules per second strike 4 cm2 of wall at an angle of 30° with the normal when moving at a speed of 2 × 103 ms−1, find the pressure exerted on the wall. (mass of one oxygen atom = 2.67 × 10−26 kg)
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)
What is an ideal gas?
Does an ideal gas exist in practice?
