Advertisements
Advertisements
प्रश्न
A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure.
(a) Find the number of moles of hydrogen present
(b) What weight of CO2can the cylinder hold under similar conditions of temperature and pressure? (H = 1 C = 12, O = 16)
(c) If the number of molecules of hydrogen in the cylinder is X, calculate the number of CO2 molecules in the cylinder with the same conditions of temperature and pressure.
(d) State the law that helped you to arrive at the above result.
Advertisements
उत्तर
(a) Given:
Mass of hydrogen = 1kg at 298K and 1 at m pressure
Moles of hydrogen = ?
Number of moles of hydrogen = `"Mass of hydrogen"/"Gram atomic mass of hydrogen"`
= `[1000 "g"]/[1 "g"]`
= 1000 moles of hydrogen
(b) Molecular mass of CO2 = 12 + 2 x 16 = 44g
So,
vapour density (VD) = `"mol. Mass"/2` = `44/2` = 22
V.D. = `"mass of certain amount of CO"_2/"mass of equal volume of hydrogen"` = `"m"/1`
22 = `"m"/1`
So, mass of CO2 = 22 Kg
(c) According to Avogadro's law, equal volumes of all gases under similar conditions of temperature and pressure contain equal number of molecules.
(d) So, number of molecules of carbon dioxide in the cylinder = number of molecules of hydrogen in the cylinder = X
APPEARS IN
संबंधित प्रश्न
Deduce the number of molecules of the following compound in the given quantity.
32g oxygen
What is the value of molar volume of a gas at S.T.P?
Calculate the mass of 0.1 mole of the following:
CaCO3
(Ca = 40, Na = 23, Mg = 24, S = 32, C = 12, Cl = 35.5, O = 16, H = 1)
Calculate the mass of 0.1 mole of the following:
Mg
(Ca = 40, Na = 23, Mg = 24, S = 32, C = 12, Cl = 35.5, O = 16, H = 1)
If phosphorus is considered to contain P4 molecules, then calculate the number of moles in 100g of phosphorus?
Correct the statement, if required.
One mole of chlorine contains 6.023 x 1010 atoms of chlorine.
From the equation for burning of hydrogen and oxygen
\[\ce{2H2 + O2 -> 2H2O}\] (Steam)
Write down the number of mole (or moles) of steam obtained from 0.5 moles of oxygen.
Solid ammonium dichromate decomposes as:
\[\ce{(NH4)2Cr2O7 -> N2 + Cr2O3 + 4H2O}\]
If 63 g of ammonium dichromate decomposes. Calculate the quantity in moles of nitrogen formed.
Match the following.
| 1. | 8 g of O2 | - | 4 moles |
| 2. | 4 g of H2 | - | 0.25 moles |
| 3. | 52 g of He | - | 2 moles |
| 4. | 112 g of N2 | - | 0.5 moles |
| 5. | 35.5 g of Cl2 | - | 13 moles |
Calculate the number of moles of magnesium present in a magnesium ribbon weighing 12 g. Molar atomic mass of magnesium is 24g mol–1.
