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December 20, 2014

Homework Help: Chemistry

Posted by Anonymous on Wednesday, July 9, 2008 at 5:40pm.

KClO3 decomposes in the presence of MnO2 to form oxygen gas, collected over H2O at 23.0 degrees C and a barometric pressure of 754.2 torr, as described in the experimental description. After the pressure of the oxygen gas is equalized with atmospheric pressure, the mass of water collected is 386.2g. If the test tube plus KCLO3 initially weighed 45.850g and had a final mass of 45.351g, answer the following questions.
1. Calculate the number of moles of oxygen generated.

2. Calculate the volume of the gas generated, from the mass and density of water displaced.

3. Calculate the pressure of dry oxygen using Dalton's law of partial pressures.

4. Calculate the value of R, the gas constant, in L atm/mole K, and in mL torr/mole K.

Please help me!

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