Advertisements
Advertisements
Question
Calculate the percent composition of Potassium chlorate KClO3.
Solution
Molecular mass of KClO3 = 122.5 g
% of K = 39 /122.5 = 31.8%
% of Cl = 35.5/122.5 = 28.98%
% of O = 3 16/122.5 = 39.18%
APPEARS IN
RELATED QUESTIONS
If the hydrogen sample contains N molecules, how many molecules are present in oxygen sample?
O2 is evolved by heating KCIO3 using MnO2 as a catalyst.
\[\ce{2KCI3 ->[MnO2] 2KCl + 3O2}\]
- Calculate the mass of KClO3 required to produce 6.72 litres of O2 at STP. [atomic masses of K = 39, Cl = 35.5, O = 16].
- Calculate the number of moles of oxygen present in the above volume and also the number of molecules.
- Calculate the volume occupied by 0.01 mole of CO2 at STP.
The equation 4NH35O2 → 4NO + 6H2O represents the catalytic oxidation of ammonia. If 100 cm3of ammonia is used, calculate the volume of oxygen required to oxidise the ammonia completely.
Give two tests of the following:
Water vapour
Concentrated nitric acid oxidizes phosphorus to phosphoric acid according to the following equation:
\[\ce{P + 5HNO3 -> H3PO4 + 5NO2 + H2O}\]
If 6.2 g of phosphorus was used in the reaction, calculate the number of moles of phosphorus taken and mass of phosphoric acid formed.
What volume of oxygen is required to burn completely a mixture of 22.4 dm3 of methane and 11.2 dm3 of hydrogen into carbon dioxide and steam?
\[\ce{CH4 + 2O2 -> CO2 + 2H2O}\]
\[\ce{2H2 + O2 -> 2H2O}\]
66g of ammonium sulphate is produced by the action of ammonia on sulphuric acid. Write a balanced equation and calculate the volume of the gas used at STP.
1.56 g of sodium peroxide reacts with water according to the following equation:
\[\ce{2Na2O2 + 2H2O -> 4NaOH + O2}\]
Calculate the volume of oxygen liberated at STP.
1.56 g of sodium peroxide reacts with water according to the following equation:
\[\ce{2Na2O2 + 2H2O -> 4NaOH + O2}\]
Calculate the mass of oxygen liberated.
Concentrated nitric acid oxidizes phosphorus to phosphoric acid according to the following equation:
\[\ce{P + 5HNO3 -> H3PO4 + 5NO2 + H2O}\]
If 6.2 g of phosphorus was used in the reaction, calculate the mass of nitric acid consumed at the same time.
