A sample of #KClO_3# on decomposition gives 448 #mL# of oxygen gas at NTP. Calculate: (a) Weight of oxygen produced (b) Weight of #KClO_3# originally taken (c) Weight of #KCl# produced?
Mass of oxygen: 0.596 g
Mass of potassium chlorate: 1.52 g
Mass of potassium chloride: 0.927 g
Start with the balanced chemical equation for the decomposition of potassium chlorate,
The important thing to notice here is that
Since you know the volume and conditions under which the oxygen gas was produced, you can use the ideal gas law equation to determine how many moles were produced.
At NTP, or Normal Temperature and Pressure, the pressure is set at 1 atm and the temperature at
Use oxygen's molar mass to determine how many grams were produced
SIDE NOTE Do not forget to convert the temperature to Kelvin and the volume to liters!
The mass of potassium chlorate that underwent decomposition can be found in a similar manner. First, determine the number of moles by using the mole ratio that exists between potassium chlorate and oxygen gas
The mass of the compound before decomposition was
The number of moles of potassium chlorate produced by the reaction will be equal to the number of moles of potassium chlorate
The mass of potassium chloride is
All three values are rounded to three sig figs, the number of sig figs you gave for the volume of oxygen gas produced.