Advertisements
Advertisements
प्रश्न
Calculate the percentage composition of oxygen in lead nitrate [Pb(NO3)2]. [Pb = 207, N= 14, O = 16]
Advertisements
उत्तर
Pb + (N)2 + (O)6
207 + 2 x 14 + 6 x 16 = 331.
So, the molecular mass of Pb(NO3)2 = 331.
331 by weight of Pb(NO3)2 contain 96 parts by weight of oxygen .
100 parts will contain = 96 x 100 / 331 = 29 ‰
So, the percentage composition of oxygen in lead nitrate is 29‰
APPEARS IN
संबंधित प्रश्न
Calculate the relative molecular mass of Sodium acetate
(use K = 39, Cl = 35.5, O = 16, C = 12, H = 1, Na = 23, N = 14, S= 32)
Calculate the percentage of boron (B) in borax (Na2B4O7.10H2O). [H = 1, B = 11, O = 16, Na = 23],
answer correct to 1 decimal place.
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)
Calculate the percentage of sodium in sodium aluminium fluoride (Na3AIF6).
[F = 19, Na = 23, Al = 27]
Give one word or phrase for the following:
Formation of ions from molecules.
Calculate the relative molecular mass of:
CHCl3
Calculate the number of hydrogen atoms in 0.1 mole of H2SO4.
Calculate the mass of nitrogen supplied to soil by 5 kg of urea [CO(NH2)2].
[O = 16; N = 14; C = 12; H = 1]
When heated, potassium permanganate decomposes according to the following equation :
\[\ce{2KMnO4 -> \underset{\text{solid residue}}{K2MnO4 + MnO2} + O2}\]
(a) Some potassium permanganate was heated in the 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.
(b) Given that the molecular mass of potassium permanganate is 158. 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)
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?
