Advertisements
Advertisements
Question
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.
Solution
\[\ce{\underset{[Steam 1 mole]}{P + 5HNO3} -> H3PO4 + H2O + 5NO2}\]
1 mole of phosphorus atom = 31 g of phosphorus
31 g of P = 1 mole of P
∴ 6.2 g of P = `(6.2 xx 1)/31`
= 0.2 mole of P
Also, 31 g of phosphorus or 1 mole of phosphorus produces H3PO4
= (3 × 1) + 31 + (4 × 16)
= 98 g of H3PO4
∴ 0.2 mole of P produces = 98 × 0.2
= 19.6 g of H3PO4
APPEARS IN
RELATED QUESTIONS
Differentiate between 2H and H2
Samples of the gases O2, N2, CO2 and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of Oxygen, occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure :
What is the volume occupied by : 3X molecules of CO? [C=12,N=14,O=16]
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.
Calculate the percentage of phosphorus in Calcium hydrogen phosphate Ca(H2PO4)2
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.
\[\ce{KNO3 + H2SO4 -> KHSO4 + HNO3}\]
\[\ce{NaNO3 + H2SO4 -> NaHSO4 + HNO3}\]
Calculate the mass of ammonia that can be obtained from 21.4 g of NH4Cl by the reaction:
\[\ce{2NH4Cl + Ca(OH)2 -> CaCl2 + 2H2O + 2NH3}\]
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?
\[\ce{CH4 + 2O2 -> CO2 + 2H2O}\]
\[\ce{2H2 + O2 -> 2H2O}\]
What mass of copper hydroxide is precipitated by using 200 gm of sodium hydroxide?
\[\ce{2NaOH + CuSO4 -> Na2SO4 + Cu(OH)2↓}\]
[Cu = 64, Na = 23, S = 32, H = 1]
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.
Aluminium carbide reacts with water according to the following equation.
\[\ce{Al4C3 + 12H2O -> 3CH4 + 4Al(OH)3}\]
What volume of methane is obtained from 12 g of aluminium carbide?
