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Root-mean-square. speed of an ideal gas:

v (rms) = sqrt(3RT/M)

where R = 8.31 J K−1·mol−1 is the gas constant, T is the absolute temperature, M the molar mass.

T = 41 + 273 = 314°K

M(chlorine) = 0.071 kg·mol−1

v (rms) = sqrt(3×8.31×314/0.071) = 332 m/s

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RE:

Calculate the root-mean-square speed of molecular chlorine in m/s at 41°C.?

I just can't figure this out... is it me or are the questions getting harder each homework problem?

V Root Mean Square

ok RMS is square root of 3RT/MM

so T = 41 + 273 = 314 K

R = 8.314

MM = 70.9 g BUT it must be in Kg so 0.0709 kg

plug into equation 3(8.314)(314)/0.0709 = 110462.45

square root that and get 332.36

The formula: V = = sqrt(3kT/m) = sqrt(3RT/M) I'm sorry but this is impossible.