(6) There is a cylindrical container with a piston with diameter d = 4.67cm which allows the volume to change. Sitting on top of that piston is a m = 6.62kg block. The temperature of the diatomic gas is T 382K and there are N = 1.45 × 1023 molecules. (a) What is the gauge pressure of the gas inside the container? (b) What is the volume of this container in cm³? (c) What is the mean free path of a molecule in this container?

(6) There is a cylindrical container with a piston with diameter d = 4.67cm which allows the volume to change. Sitting on top of that piston is a m = 6.62kg block. The temperature of the diatomic gas is T 382K and there are N = 1.45 × 1023 molecules. (a) What is the gauge pressure of the gas inside the container? (b) What is the volume of this container in cm³? (c) What is the mean free path of a molecule in this container?

Similar questions

The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV = nRT, where n is the number of moles of the gas and R = 0.0821 is the gas constant. Suppose that, at a certain instant, P = 9.0 atm and is increasing at a rate of 0.15 atm/min and V = 13 L and is decreasing at a rate of 0.17 L/min. Find the rate of change of T with respect to time at that instant if n = 10 mol. (Round your answer to four decimal places.) K/min dT_ dt
The total translational kinetic energy of the molecules of a sample of gas at 415 K is 17500 J. How many moles n does the sample comprise? mol n = Find the average translational kinetic energy Ky of a single molecule. J Kav
a 6.0 cm diameter cyliinder of nitrogen gas has a 4.0 cm thick movable copper piston. the cylinder is oriented vertically as shown in the figure, and the air above the piston is evacuated. when the gas temperature is 25 degree C the piston floats 20 cm above the bottom of the cylinder what is the gas pressure? how many gas molecules are in the cylinder?
The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV = nRT, where n is the number of moles of the gas and R = 0.0821 is the gas constant. Suppose that, at a certain instant, P = 9.0 atm and is increasing at a rate of 0.15 atm/min and V = 13 L and is decreasing at a rate of 0.17 L/min. Find the rate of change of T with respect to time at that instant if n = 10 mol. (Round your answer to four decimal places.) dT=0.512 dt X K/min
n = 3.8 moles of an ideal gas are pumped into a chamber of volume V= (0.083 m³. The initial pressure of the gas is 1.01 × 10° Pa (about 1 atm). What is the initial temperature, in kelvin, of the gas? T = The pressure of the gas is increased ten times. Now what is the temperature, in kelvin, of the gas? T =
A sample of carbon dioxide (CO₂) has a volume of 0.04 m³. The gas has a pressure of 1.6 x 106 Pa and its temperature is 24 degrees C. List of atomic mass units can be found HERE a) What is the mass of the whole sample of gas? b) How many molecules are in the cylinder? c) What is the average kinetic energy per molecule? d) What is the rms speed of the molecules?
Problem 5: n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.094 m3. Part (a) The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas? 50% Part (b) The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas?
Two containers of equal volume each hold samples of the same ideal gas. Container A has 2 times as many molecules as container B. If the gas pressure is the same in the two containers, find the ratio of the the absolute temperatures TA and TB ( i.e TA / TB ) . Calculate to 2 decimals.