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 |
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:
The natural isotopic abundance of 10B is 19.60% and 11B is 80.40 %. The exact isotopic masses are 10.13 and 11.009 respectively. Calculate the average atomic mass of boron
What is the mass of precipitate formed when 50 ml of 8.5% solution of AgNO3 is mixed with 100 ml of 1.865% potassium chloride solution?
Define relative atomic mass.
Boron has two isotopes 10B and 11B with atomic masses 10 and 11, respectively. If its average atomic mass is 10.81, the abundance of 10B is ____________.
How many moles of ammonia are present in 5.6 cm3 of ammonia gas at STP?
What is the average mass of an element if it has two isotopes, one of mass 6.015 u with 8.24 % and other of mass 7.016 u with 91.26% respectively?
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 ______.
