Advertisements
Advertisements
Question
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
Solution
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
RELATED QUESTIONS
Calculate the molecular mass of the following in u.
NH3
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.
24 g of carbon reacts with some oxygen to make 88 grams of carbon dioxide. Find out how much oxygen must have been used.
Which one of the following is used as a standard for 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 ____________.
The unit of atomic mass, amu is replaced by u, here u stands for ______.
Calculate mass of 3.01 × 1024 atoms of an element having atomic mass 21.13.
A 100 g of sample of haemoglobin on analysis was found to contain 0.34% Fe by mass. If each haemoglobin molecule has four Fe2+ ions, the molecular mass of haemoglobin is: (Fe = 56 amu)
Which symbol replaces the unit of atomic mass, amu?
