Advertisements
Advertisements
प्रश्न
When heated, potassium permanganate decomposes according to the following equation:
\[\ce{2KMnO4 -> \underset{solid residue}{K2MnO4 + MnO2} + O2}\]
Given that the molecular mass of potassium permanganate is 158 g, what volume of oxygen (measured at room temperature) would be obtained by the complete decomposition of 15.8 g of potassium permanganate? (Molar volume at room temperature is 24 litres). [K = 39, Mn = 55, O = 16]
Advertisements
उत्तर
| 2KMnO4 | → | K2MnO4 | + | MnO2 | + | O2 |
| 2[39 + 55 + 64] | 24 lit | |||||
| 2 × 158 = 316 g |
Vol. of O2 produced by 316 g of KMnO4 = 24 lit.
∴ Vol. of O2 produced by 15.8 of KMnO4 = `(24 xx 15.8)/316`
= 1.2 lit.
संबंधित प्रश्न
Calculate the relative molecular mass of Potassium chlorate.
(use K = 39, Cl = 35.5, O = 16, C = 12, H = 1, Na = 23, N = 14, S=32)
Concentrated nitric acid oxidizes phosphorous to phosphoric acid according to the following equation :
P + 5HNO3 → H3PO4 + H2O + 5NO2
What mass of phosphoric acid can be prepared from 6 .2 g of phosphorous?
Calculate the percentage of phosphorous in the fertilizer superphosphate, Ca(H2PO4)2. [Ca = 40, H =1, P =31, O = 16] (Correct to 1 decimal place)
A compound 'X' consists of 4.8% of C and 95.2% of Br by mass.
Name the type of chemical reaction by which X can be prepared from ethane.
Give two tests of the following:
Oxygen
Calculate the relative molecular mass of:
Ammonium chloroplatinate (NH4)2 PtCl6
The mass of 5.6 litres of a certain gas at S.T.P. is 12 g. What is the relative molecular mass or molar mass of the gas?
Calculate the mass of nitrogen supplied to soil by 5 kg of urea [CO(NH2)2].
[O = 16; N = 14; C = 12; H = 1]
A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure. What mass of carbon dioxide can it hold under similar conditions of temperature and pressure?
Ammonia burns in oxygen and the combustion, in the presence of a catalyst, may be represented by;
\[\ce{2NH3 + 2 1/2O2 -> 2NO + 3H2O}\] [H = 1, N = 14, O = 16]
What mass of steam is produced when 1.5 g of nitrogen monoxide is formed?
