The velocities of five molecules are 2 m/s, 3 m/s, 4 m/s, 5 m/s + 6m/s resp. Find the mean velocity and the root mean square velocity of the molecules.

The following figure is a histogram showing the speeds of the molecules in a very small gas. What are (a) the most probable speed, (b) the average speed, and (c) the rms speed?

ASAP

The rms average speed of a nitrogen molecule at 20 K is 133.427875 m/s. What is the rms average speed at 80 K?

What is the root mean squared velocity of Nitrogen gas at room temperature (295 K)? The mass of N2 is 4.65 x 10-26 kg. Is every gas molecule moving at this speed?

A glass container encloses a low pressure of 02 gas at 298 K. The molecular weight of 02 is 32.0 g/mol.  (A) Calculate the mean squared velocity, v², of these molecules in units of m²/s². (B) Find the root mean squared speed along the x-axis, Vx. (C) Would Vx be lower, higher, or the same under the same conditions if the gas were He instead of 02? Please explain your answer in 15 words or less.

Show that the rms speed of molecules in a gas is given by ЗР Vrms where P is the pressure in the gas, and p is the gas density.

A room is 10.0 m by 7.5 m by 2.7 m is filled with air at 22oC and 1 atm. The average molar mass of air is 28.8 g/mol. Find the number of moles of air to fill the room and the weight of the air in kg.

The root mean square velocity of an oxygen molecule is 1,302.27 m/s. Estimate the temperature at which it is located.

Find the total number of collisions between molecules in 1.00 s in 1.00 L of nitrogen gas at standard temperature and pressure ( 0 °C , 1.00 atm). Use 1.88 × 10−10 m as the effective radius of a nitrogen molecule. (The number ofcollisions per second is the reciprocal of the collision time.) Keep in mind that each collision involves two molecules, so if one molecule collides once in a certain period of time, the collision of the molecule it hit cannot be counted.