An unknown diatomic gas effuses at a rate that is 0.250 times the rate of N2 at the same temperature. What is the Molar mass and identity of the gas?
2006-11-10 08:57:49 · 3 answers · asked by uf2006mvp 1 in Science & Mathematics ➔ Chemistry
Rate of effusion for gas 1 / rate of effusion for gas 2 = sqrt M2 / sqrt M1 (where M is molar mass)
2006-11-10 09:13:01 · answer #1 · answered by scurvybc 3 · 0⤊ 0⤋
If effuses is a typo for diffuses then the rate varies like the square root of the masses
2006-11-10 09:10:02 · answer #2 · answered by meg 7 · 0⤊ 1⤋
enable fee of effussion of unknown gas be r1 and that of NO2 be r2 so r1/r2 = sq. root of ( molecular mass of NO2/molecular mass of unknown gas) 0.80 5 = sq. root of ( 40 six/molecular mass of unknown gas) squaring the two sides ... 40 six/molecular mass of unknown gas = 0.80 5^2 40 six/molecular mass of unknown gas = 0.7225 molecular mass of unknown gas = 40 six/0.7225 = sixty 3.667 g/mole
2016-12-14 04:59:21 · answer #3 · answered by karsten 4 · 0⤊ 0⤋