Calculate the rms speed of an oxygen gas molecule, O2, at 17.0 C Express your an

Question

Calculate the rms speed of an oxygen gas molecule, O2, at 17.0 C Express your answer numerically in meters per second Constants Periodic Table View Available Hint(s) Learning Goal To calculate the rms speed and relative rates of effusion of gas molecules In a given sample of gas, the particles move at varying speeds. The root mean square speed (rms speed) of particles in a gas sample, u, is given by the formula m/s Submit where T is the Kelvin temperature, M is the molar mass in kg/mol, and R = 8.314 J/(mol·K) is the gas constant. Effusion is the escape of gas molecules through a tiny hole into a vacuum. The rate of effusion of a gas is directly related to the rms speed of the gas molecules, so it's inversely proportional to the square root of its mass. The rms speed is related to kinetic energy, rather than average speed, and is the speed of a molecule possessing a kinetic energy identical to the average kinetic energy of the sample. Given its relationship to the mass of the molecule, you can conclude that the lighter the molecules of the gas, the more rapidly it effuses. Mathematically, this can be expressed as Part B Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them View Available Hint(s) Reset Help effusion rate ox TrL The relative rate of effusion can be expressed in terms of molecular masses RA and TLB as

Explanation / Answer

part-A

molar mass of O2 = 32 gram/mole = 0.032 Kg/mole

R= 8.314J

T= 17C= 17+273= 290K

RMS velocity = square root of 3RT/M

RMS velocity = square root 3x 8.314x290/0.032

                     = 475.43m/s

RMS velocity of O2 = 475.4 m/s

2.

H2 > Ne>CO > Ar > C3H8

molar mass of H2= 2g/mole

molar mass of Ne = 20 g/mole

molr mass of CO=28 g/mole

molae mass 0f Ar=39.9 g/mole

molar mass of C3H8= 44 g/mole

H2 has less mass ; so it has high rate of diffusion

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