Chemistry
Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation:
P + 5HNO3 [conc.] ⟶ H3PO4 + H2O + 5NO2.
If 9.3 g of phosphorus was used in the reaction, calculate :
(i) Number of moles of phosphorus taken.
(ii) The mass of phosphoric acid formed.
(iii) The volume of nitrogen dioxide produced at STP.
Related Questions
An organic compound has vapour density 94. It contains C = 12.67%, H = 2.13%, and Br = 85.11%. Find the molecular formula of the organic compound.
[C = 12, H = 1, Br = 80]
Calculate the mass of :
(i) 1022 atoms of sulphur.
(ii) 0.1 mole of carbon dioxide.
[S = 32, C = 12 and O = 16 and Avogadro's Number 6 × 1023]
67.2 litres of H2 combines with 44.8 litres of N2 to form NH3 :
N2(g) + 3H2(g) ⟶ 2NH3(g).
Calculate the vol. of NH3 produced. What is the substance, if any, that remains in the resultant mixture ?
The mass of 5.6 dm3 of a certain gas at STP is 12.0 g. Calculate the relative molecular mass of the gas.