A sample of hydrogen gas has a density of -g at a pressure of 1.06 atm and a tem

Question

A sample of hydrogen gas has a density of -g at a pressure of 1.06 atm and a temp of 56 degree C? Assume ideal behavior. A sample of an unknown gas is found to have a density of 2.27 g/L at a pressure of 0.864 atm and a temp at 38 degree C. The molecular weight of the unknown gas is - g/mol. The average molecular speed is a sample of so_2, gas at a certain temp is 34 m/s. the average molecular speed in a same temp. The rate of effusion of OH_3 gas through a porous barrier is observed to be 8.09 times 10^-4 mol/n. Under the same conditions the rate of effusion of O_2 gas would be - mol/n.

Explanation / Answer

(1) P V = n R T

P V = (m/M) R T

M P = (m/V) R T

M P = d R T

For ideal gas,

d = M*P / R T = 2 * 1.06 / (0.0821*329.15) = 0.07845 g/L

(2) M = d R T / P = 2.75 * 0.0821 *311.15 / 0.844 = 83.2 g/mol

(3) According to kinetic molecular theory of gases,

r1/r2 = sqrt.(M2/M1)

348 / r2 = sqrt. (83.80 / 64)

r2 = average velocity of Kr gas = 304.2 m/s

(4) According to graham's law of diffusion,

r1/r2 = sqrt.(M2/M1)

(8.09*10-4)/r2 = sqrt.(32/17)

r2 = 8.09*10-4/1.372 = 5.896*10-4 m/s

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