Bath Temperture 34.0 degrees C Total Volume of O2 collected is 18.0 mL Barametri

Question

Bath Temperture 34.0 degrees C

Total Volume of O2 collected is 18.0 mL

Barametric Pressure 760 mm Hg

Vapor pressure of water at bath temperature is 39.9 mm Hg

Slope: 0.0658

Using the ideal-gas law, calculate the moles of O2 collected _____________ mol O2.

I am looking for step by step instructions so that I can understand this procedure for further exams. Thanks in advance.

Buret Reading (mL) Vol of O2 (mL) Time in seconds 4.5 0 0 6.5 2.0 10 8.5 4.0 36 10.5 6.0 87 12.5 8.0 119 14.5 10.0 150 16.5 12.0 178 18.5 14.0 203 20.5 16.0 228 22.5 18.0 256

Explanation / Answer

Volume of O2 collected = 0.018 litres

Pressure exerted by O2 = barometric pressure - vapor pressure of water = 720.1 mm Hg = 0.9475 atm

Applying Ideal Gas Equation; i.e.

P*V = n*R*T we get

0.9475*0.018 = n*0.0821*(273+34)

or, n = moles of O2 = 6.767*10-4

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