If potassium chlorate is 80% pure, then 48 g of oxygen would be produced from (atomic mass of K = 39)

Calculate the mass of potassium chlorate which will produce 24 g of oxygen on complete decomposition. Also calculate the mass of potassium chloride formed. (K = 39, O = 16)

What mass of potassium chlorate must be decomposed to produce 2.40 L of oxygen at 0.82 "bar" and 300 K ?

What mass of potassium chlorate must be decomposed to produce 2.40 L of oxygen at 0.82 "bar" and 300 K ?

6g of an impure sample of potassium chlorate gives 1.9g of oxygen on heating in presence of a catalyst. What is the percentage of purity of the sample. [K = 39,Cl = 35.5, O = 16]

How much potassium chlorate should be heated to produce 2.24L of oxygen at NTP?

Calculate the mass of potassium chlorate required to librate 6.72 dm^3 of oxygen at STP, molar mass of potassium chlorate is 122.5 g /mol .

Compute the mass of potassium chlorate (KClO_(3)) that should decompose to produce 8 g of oxygen as per the chemical equation , 2KClO_(3) to 2KCl + 3O_(2)(g) (R.A.M : K = 39, Cl = 35.5,O = 16 .)

Potassium chlorate decomposes, on heating, to form potassium chloride and oxygen. When 24.5 g of potassium chlorate is decomposed completely, then 14.9g of potassium chloride is formed. Calculate the mass of hydrogen formed. Which law of chemical combination have you used in solving this problem ?