Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation: P+5HNO3→H3PO4+5NO2+H2O If 6.2 g of phosphorus was used in the reaction, calculate:
(a) The number of moles of phosphorus taken and mass of phosphoric acid formed. (b) Mass of nitric acid consumed at the same time. (c) The volume of steam produced at the same time if measured at 760 mm Hg pressure and 273∘C.
(a) Concentrated nitric acid oxidises phosphorus to phosphoric acid according to the following equation: P + 5HNO3 → H3PO4 + H2O + 5NO2 (i) What mass of phosphoric acid can be prepared from 6.2 g of phosphorus? (ii) What mass of nitric acid will be consumed at the same time? (iii) What will be the volume of steam at the same time measured at 760 mm Hg pressure and 373°C? (H = 1; N = 14; O = 16; P = 31) (b) Ammonia may be oxidised to nitrogen monoxide in the presence of a catalyst according to the following equation: 4NH3 + 5O2 → 4NO + 6H2O If 27 litres of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature and pressure?