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प्रश्न
Prove the Following :
Oxygen is a diatomic molecule.
उत्तर
Since one Oxygen molecule contains 2 atoms of oxygen, so it is a diatomic molecule.
O + O → O2
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संबंधित प्रश्न
Give three pieces of information conveyed by the formula H2O.
The ratio between the number of molecules in 2g of hydrogen and 32 g of oxygen is
[Given that H=1,O=16]
The reaction between the red lead and hydrochloric acid is given below:
\[\ce{Pb3O4 + 8HCl -> 3PbCl2 + 4H2O + Cl2}\]
Calculate the mass of lead chloride formed by the action of the 6.85 g of red lead.
Find the mass of KNO3 required to produce 126 kg of nitric acid. Find whether a larger or smaller mass of NaNO3 is required for the same purpose.
\[\ce{KNO3 + H2SO4 -> KHSO4 + HNO3}\]
\[\ce{NaNO3 + H2SO4 -> NaHSO4 + HNO3}\]
Aluminium carbide reacts with water according to the following equation.
\[\ce{Al4C3 + 12H2O -> 3CH4 + 4Al(OH)3}\]
What mass of aluminium hydroxide is formed from 12g of aluminium carbide?
Calculate the mass of ammonia that can be obtained from 21.4 g of NH4Cl by the reaction:
\[\ce{2NH4Cl + Ca(OH)2 -> CaCl2 + 2H2O + 2NH3}\]
Solid ammonium dichromate decomposes as:
\[\ce{(NH4)2Cr2O7 -> N2 + Cr2O3 + 4H2O}\]
If 63 g of ammonium dichromate decomposes. Calculate the volume of N2 evolved at STP.
Pure calcium carbonate and dilute hydrochloric acid are reacted and 2 litres of carbon dioxide were collected at 27°C and normal pressure.
\[\ce{CaCO3 + 2HCl -> CaCl2 + H2O + CO2}\]
Calculate the mass of the acid required.
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.
Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
\[\ce{P + 5HNO3_{(conc.)}-> H3PO4 + H2O + 5NO2}\]
If 9.3 g of phosphorus was used in the reaction, calculate:
- Number of moles of phosphorus taken.
- The mass of phosphoric acid formed.
- The volume of nitrogen dioxide produced at STP.
