while you are answering, can ypu please right the steps ofcalculations and how you solve it.
1)a 1.7892 g sample of a KCLO (3) -KCL mixture is stronglyheated. All of the KCLO(3) in the mixture undergoes decomposition.The potassium chloride from the original sample plus the KCLgenerated by the reaction above weighted 1.6633 g. The gasgenerated from the reaction was collected over water and a volumeof 113.6 ml. at 24.0 C was obtained. The barometric pressure was647 mm Hg.
a)Determine the mass of O(2) evolved by using gravimetric(weight based) measurements. Do not use the ideal gas law.
b)How many moles of O(2) gas were evolved?
c)How many g of potassium chloride were inthe original?
d)What % of KCLO(3) was in the original sample?
e)Assuming no O(2) dissolved in the water over which it wascollected, calculate the volume of O(2), collected under standartconditions (o.celcium 760 mm). remember that pressure of O(2) overthe water must be calculated from the baromatric pressure aftertaking into consideration the vapor pressure of water.
f)take the ration part e/part b . This is the molar volume(l/mole) How does this value compare to the molar volume of anideal gas?