a 1.2475 g sample of a KCIO3 - KCI mixture is strongly heated. All of the KCI3 in the mixture undergoes decomposition. The potassium chloride from the original sample plus the KCI generated by the reaction above weighed 1.0596 g. The gas generated from the reaction was collected over water and a volume of 192 mL at 24C was obtained. the barometric pressure was 645 mm Hg.
a) dtermine the mass of O2 evolved by using gravimetric ( weight based ) measurments. Do not use ideal gas law.
b) How many moles of gas were evolved?
c) how many grams of potassium chlorate were in the original mixture?
d) what percent of KCIO3 was in the priginal sample?
e) Assuming no O2 dissolved in the water over which it was collected, calculate the volume of O2 collected under standard conditions (O degress Celsius and 760 mm Hg). Remember that the pressure of O2 over water must be calculated from the barometric pressure after taking into consideration the vapor pressure of water.
f) Take the ration of part e/part b. This is the molar volume (L/mole). How does this value compare to the molar volume of an ideal gas?