Advertisements
Advertisements
प्रश्न
Calculate the volume of oxygen required for the complete combustion of 8.8 g of propane (C3H5).
(Atomic mass: C = 14, O = 16, H = 1, Molar Volume = 22.4 dm3 at STP.)
Advertisements
उत्तर
\[\ce{C3H8 + 5O2 -> 3CO2 + 4H2O}\]
Molar weight of propane = 12 × 3 + 8 = 44
Volume of 5O2 = 5 × 22.4 = 112 litres
44 g of propane requires = 112 litres of oxygen
1 g of propane requires = `112/44` litres
8.8 g of propane requires = `112/44 xx 8.8`
= 112 × 0.2
= 22.4 litres
APPEARS IN
संबंधित प्रश्न
What is the mass of nitrogen in 1000Kg of urea [CO(NH2)2] ?
[H = 1, C= 12, N= 14, O = 16]
Water can split into hydrogen and oxygen under suitable conditions. The equations representing the change is: 2H2O(I) → 2H2 (g) + O2(g)
Ammonia burns in oxygen and the combustion in the presence of a catalyst may be represented as:
2NH3 (g) +21/2O2 (g) → 2NO (g) + 3H2O (I)
What mass of steam is produced when 1.5 g of nitrogen monoxide is formed?
Calculate the percentage of platinum in ammonium chloroplatinate (NH4)2PtCl6.
[N = 14, H = 1, Pt = 195, Cl =35.5]
(Give your answer correct to the nearest whole number)
The reaction of potassium permanganate (VII) with acidified iron (II) sulphate is given below:
2KMno4 + 10FeSO4 + 8H2O → K2SO4 + 2MnSO4 + 5Fe2(SO4)3 + 8H2O
If 15.8g of potassium permanganate (VII) was used in the reaction, calculate the mass of iron (II) sulphate used in the above reaction.
When heated, potassium permanganate decomposes according to the following equation:
\[\ce{2KMnO4 -> \underset{solid residue}{K2MnO4 + MnO2} + O2}\]
Some potassium permanganate was heated in test tube. After collecting one litre of oxygen at room temperature, it was found that the test tube had undergone a loss in mass of 1.32 g. If one litre of hydrogen under the same conditions of temperature and pressure has a mass of 0.0825 g, calculate the relative molecular mass of oxygen.
Calculate the percentage of nitrogen in aluminium nitride. [Al = 27, N = 14]
Calculate the relative molecular mass of:
Potassium chlorate
Which of the following would weigh most?
The following question refers to one mole of chlorine gas.
If the relative atomic mass of chlorine is 35.5, what will be the mass of 1 mole of chlorine gas?
67.2 litres of hydrogen combines with 44.8 litres of nitrogen to form ammonia under specific conditions as:
\[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\]
Calculate the volume of ammonia produced. What is the other substance, if any, that remains in the resultant mixture?
