Advertisements
Advertisements
प्रश्न
Calculate the average atomic mass of naturally occurring magnesium using the following data.
| Isotope | Isotopic atomic mass | Abundance (%) |
| Mg24 | 23.99 | 78.99 |
| Mg25 | 24.99 | 10.00 |
| Mg26 | 25.98 | 11.01 |
Advertisements
उत्तर
Average atomic mass = `((78.99 xx 23.99) + (10 xx 24.99) + (11.01 xx 25.98))/100`
= `2430.9/100`
= 24.31 u
APPEARS IN
संबंधित प्रश्न
The number of molecules in 22.4 cm3 of nitrogen gas at STP is ______.
Calculate the molecular mass of the following in u.
CH3COOH
Solve problem:
Arjun purchased 250 g of glucose (C6H12O6) for Rs 40. Find the cost of glucose per mole.
Solve problem:
Calculate the number of moles of magnesium oxide, MgO in
- 80 g, and
- 10 g of the compound.
(Average atomic masses of Mg = 24 and O = 16)
Explain the need of the term average atomic mass.
Which one of the following represents 180 g of water?
Which one of the following is used as a standard for atomic mass.
The reaction between aluminium and ferric oxide can generate temperatures up to 3273 K and is used in welding metals.
(Atomic mass of Al = 27 u Atomic mass of O = 16 u)
\[\ce{2Al + Fe2O3 -> Al2O3 + 2Fe}\]; If, in this process, 324 g of aluminium is allowed to react with 1.12 kg of ferric oxide.
- Calculate the mass of Al2O3 formed.
- How much of the excess reagent is left at the end of the reaction?
Calculate mass of 3.01 × 1024 atoms of an element having atomic mass 21.13.
It is found that in 11.2 L at 0°C and 1 atm, of any gaseous compound of 'X', there is never less than 15.5 gm of 'X'. It is also found that 11.2 L of vapours of 'X' at 0°C and 1 atm, weighs 62 gm. The atomicity of 'X' is ______.
