You blow up a spherical balloon to a diameter of 50.0 cm until the absolute pressure inside is 1.25 atm and the temperature is 22.0C. Assume that all the gas is N2, of molar mass 28.0 g>mol. (a) Find the mass of a single N2 molecule. (b) How much translational kinetic energy does an average N2 molecule have? (c) How many N2 molecules are in this balloon? (d) What is the total translational kinetic energy of all the molecules in the balloon?

You blow up a spherical balloon to a diameter of 50.0 cm until the absolute pressure inside is 1.25 atm and the temperature is 22.0C. Assume that all the gas is N2, of molar mass 28.0 g>mol. (a) Find the mass of a single N2 molecule. (b) How much translational kinetic energy does an average N2 molecule have? (c) How many N2 molecules are in this balloon? (d) What is the total translational kinetic energy of all the molecules in the balloon?

Similar questions

The mean free path is the average distance traveled by a particle between collisions with other particles. Calculate the mean free path of air at room temperature, T = 67.0 °F. Air is mostly nitrogen, so assume that the collisions are between moving N₂ molecules. The diameter of N₂ is d = 1.87 × 10−¹0 m and the gas is at atmospheric pressure, P = 101325 Pa. λ = m
Nitrogen gas is at 300° C temperature. The temperature (in K) at which the rms speed of a H2 molecule would be equal to the rms speed of a nitrogen molecule, is _________. (Molar mass of N2 gas 28 g).
The mean free path is the average distance traveled by a particle between collisions with other particles. Calculate the mean free path ? of air at room temperature, ?=60.0 ∘F. Air is mostly nitrogen, so assume that the collisions are between moving N2 molecules. The diameter of N2 is ?=1.00×10−10 m and the gas is at atmospheric pressure, ?=101325 Pa.
You have a container of neon (Ne) gas at 290 K. The volume of the container is 0.1 m3 and the pressure is 2.1 atm. a) How many Ne atoms are in the container? b) How many moles of Ne are in the container?
On a chilly 10°C day, you quickly take a deep breath—all your lungs can hold, 4.0 L. The air warms to your body temperature of 37°C. If the air starts at a pressure of 1.0 atm, and you hold the volume of your lungs constant (a good approximation) and the number of molecules in your lungs stays constant aswell (also a good approximation), what is the increase in pressure inside your lungs?
What is the average translational kinetic energy of 1 mole of monatomic ideal gas that has a temperature of 50 degrees Celsius. (R = 8.314 J/mol K, k =1.381 x 10^-23 J/molecule K) O 5190 J O 624 J 4030 J 985 J
Mercury boils at 357°C and freezes at –38.9°C. a. Convert these temperatures to Kelvin.
The rms speed of the molecules of a gas at 133°C is 195 m/s. Calculate the mass m of a single molecule in the gas. kg m =
Oxygen (O2, with molar mass 32.0 g/mol) gas at 269 K and 1.02 atm is confined to a cubical container 9.50 cm on a side. Calculate ΔUg/Kavg, where ΔUg is the change in the gravitational potential energy of an oxygen molecule falling the height of the box and Kavg is the molecule's average translational kinetic energy.