Advertisements
Advertisements
Question
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?
Solution
\[\ce{Al4C3 + 12H2O -> 3CH4 + 4Al(OH)3}\]
[4 x 27 + 3 x 12] 4[27 + 17 x 3]
108 + 36 4[27 x 51]
144 g 312 g
Since 144 g of Al4C3 gives 312g of Al(OH)3
So , 12 g of Al4C3 will give = `312/144 xx 12`
= 26 g Al(OH)3
APPEARS IN
RELATED QUESTIONS
Oxygen oxidises ethyne to carbon dioxide and water as shown by the equation:
\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]
What volume of ethyne gas at STP required to produce 8.4 dm3 of carbon dioxide at STP?
[H = 1, C = 12, O = 16]
Give three pieces of information conveyed by the formula H2O.
What volume of oxygen is required to burn completely a mixture of 22.4 dm3 of methane and 11 .2 dm3 of hydrogen in to carbon dioxide and steam? Equations of the reactions are given below:
CH4 + 2O2 → CO2 + 2H2O
2H2 + O2 → 2H2O
LPG stands for liquefied petroleum gas. Varieties of LPG are marketed including a mixture of propane (60%) and butane (40%). If 10 litres of this mixture is burnt, find the total volume of carbon dioxide gas added to the atmosphere. Combustion reaction can be represented as:
\[\ce{C3H8_{(g)} + 5O2_{(g)} -> 3CO2_{(g)} + 4H2O_{(g)}}\]
\[\ce{2C4H10_{(g)} + 13O2_{(g)} -> 8CO2_{(g)} + 10H2O_{(g)}}\]
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 volume of oxygen at STP required for the complete combustion of 100 litres of carbon monoxide at the same temperature and pressure.
\[\ce{2CO + O2 → 2CO2}\]
The reaction between 15 g of marble and nitric acid is given by the following equation:
\[\ce{CaCO3 + 2HNO3 -> Ca(NO3)2 + H2O + CO2}\]
Calculate the volume of carbon dioxide evolved at S.T.P.
1.56 g of sodium peroxide reacts with water according to the following equation:
\[\ce{2Na2O2 + 2H2O -> 4NaOH + O2}\]
Calculate the mass of sodium hydroxide formed.
66g of ammonium sulphate is produced by the action of ammonia on sulphuric acid. Write a balanced equation and calculate the mass of acid required.
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.
