Reference no: EM132815139

Problem 1: Calculate the rms speed of a nitrogen molecule at room temperature.

Problem 2: If you poke a hole in a container full of gas, the gas will start leaking out. In this problem you will make a rough estimate of the rate at which gas escapes through a hole. (This process is called effusion, at least when the hole is sufficiently small.)

(a) Consider a small portion (area = A) of the inside wall of a container full of gas. Show that the number of molecules colliding with this surface in a time interval Δt is PAΔt/(2m‾v_x), where P is the pressure, m is the average molecular mass, and v_x is the average x velocity of those molecules that collide with the wall.

(b) Its not easy to calculate ‾v_x, but a good enough approximation is (‾v²_x)^1/2, where the bar now represents an average over all molecules in the gas. Show that (v_x²)1/2 = √(kT/m).

(c) If we now take away this small part of the wall of the container, the mole¬cules that would have collided with it will instead escape through the hole. Assuming that nothing enters through the hole, show that the number N or molecules inside the container as a function of time is governed by the differential equation

dN/dt = - A/2V √kT/m N.

Solve this equation (assuming constant temperature) to obtain a formula of the form N(t) = N(0)e^-t/τ, where τ is the "characteristic time" for N (and P) to drop by a factor of e.

(d) Calculate the characteristic time for air at room temperature to escape from a 1-liter container punctured by a 1-mm² hole.

(e) Your bicycle tire has a slow leak, so that it goes flat within about an hour after being inflated. Roughly how big is the hole? (Use any reasonable estimate for the volume of the tire.)

In Jules Verne's Round the Moon, the space travelers dispose of a dog's corpse by quickly opening a window, tossing it out, and closing the window. Do you think they can do this quickly enough to prevent a significant amount of air from escaping? Justify your answer with some rough esti¬mates and calculations.

Problem 3: Calculate the total thermal energy in a liter of helium at room temperature and atmospheric pressure. Then repeat the calculation for a liter of air.

Problem 4: Calculate the total thermal energy in a gram of lead at room temperature, assuming that none of the degrees of freedom are "frozen out" (this happens to be a good assumption in this case).