Estimating the collision time in a helium-filled chamber at a pressure of 4×10-11Pa is a complex problem, and it requires some knowledge of gas laws and kinetic theory. However, we can break it down into smaller steps to make it more manageable.
First, we need to understand the concept of collision time. It is the average time between collisions of gas molecules in a chamber. In other words, it is the time it takes for a molecule to travel from one end of the chamber to the other and collide with another molecule.
To estimate the collision time, we need to know the average speed of the helium molecules in the chamber. According to the kinetic theory of gases, the average speed of a gas molecule is given by the formula:
v = √(3RT/M)
Where v is the average speed, R is the gas constant, T is the temperature in Kelvin, and M is the molar mass of the gas.
In this case, we have helium gas at a temperature of 380K. The molar mass of helium is approximately 4g/mol. Plugging these values into the formula, we get an average speed of 1,506 m/s.
Next, we need to calculate the mean free path of the helium molecules. This is the average distance a molecule travels between collisions. It is given by the formula:
λ = (kT)/(√2πd^2P)
Where λ is the mean free path, k is the Boltzmann constant, T is the temperature in Kelvin, d is the diameter of the molecule, and P is the pressure.
In this case, we have a pressure of 4×10-11Pa and a diameter of 1×10-10m. Plugging these values into the formula, we get a mean free path of 8.2×10-7m.
Finally, we can calculate the collision time using the formula:
tau = λ/v
Substituting the values we calculated, we get a collision time of 5.4×10-10s or 0.54 nanoseconds.
In conclusion, estimating the collision time in a helium-filled chamber at a pressure of 4×10-11Pa is a complex problem, but by breaking it down into smaller steps and using the formulas of kinetic theory, we can estimate it to be approximately 0.54 nanoseconds.
