Before reaction: a. unknown number b. weight of beaker, test tube weight of beak

Question

Before reaction: a. unknown number b. weight of beaker, test tube weight of beaker, test tube, KCIO3 KCI qui d. weight of beaker, test tube, KCIO3 -KCI, Mno2 e. weight of KCIO3 KCI ple (c-b) After reaction: 604mi f. volume of oxygen collected at laboratory temperature and pressure 246.3 n (determined by the amount of water expelled from the flask g. temperature of the oxygen h. water vapor pressure at the measured temperature (table: Handbook of Chemistry and Physics) 750mm i. barometric pressure H j. pressure of oxygen collected li-h) k. weight of beaker, test tube, Mno2 residue 0.39 CALCULATIONS I. Using the following steps with the proper number of significant figures, calculate the molar volume of oxygen showing all work clearly. O m O A. the moles of oxygen gas formed (use mass of gas from l) 3 q 3 umol 32.0 129 Nirode

Explanation / Answer

Following is the solution to Question - 1 and Question - 2 respectively.

Solution to Question - 1:

  Since here Oxygen (i.e. O2 ) pushes water from the Florence Flask into the Beaker, through the syphon, the apparatus is allowed to cool to room temperature, before the syphon between the Florence Flask and the Beaker is disconnected, most probably to measure the volume of produced/formed Oxygen (i.e. O2 ) at room temperature accurately, by measuring the volume of water collected in the Beaker.

Solution to Question - 2 :

  I think the latter, i.e. calculating moles of Oxygen from the weight of Oxygen generated, would be more accurate, because if one was to calculate the moles (assuming the use of the ideal gas equation), one would need the pressure, temperature, and the volume. Therefore, there is a big chance of getting erroneous values as you measure all the three, while calculating the moles of Oxygen formed from volume of O2 formed at STP.

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