Advertisements
Advertisements
Question
Calculate the average atomic mass of hydrogen using the following data:
| Isotope | % Natural abundance | Molar mass |
| 1H | 99.985 | 1 |
| 2H | 0.015 | 2 |
Advertisements
Solution
Average Atomic Mass = `({("Nautral abundance of" ^1"H" xx "molar mass") + ("Natural abundance of" ^2"H" xx "molar mass of" ^2"H")})/100`
= `(99.985 xx 1 + 0.015 xx 2)/100`
= `(99.985 + 0.030)/100`
= `100.015/100`
= 1.00015 u
APPEARS IN
RELATED QUESTIONS
Calculate the atomic mass (average) of chlorine using the following data :-
| % Natural Abundance | Molar Mass | |
| 35Cl | 75.77 | 34.9689 |
| 37Cl | 24.23 | 36.9659 |
Two students performed the same experiment separately and each one of them recorded two readings of mass which are given below. Correct reading of mass is 3.0 g. On the basis of given data, mark the correct option out of the following statements.
| Student | Readings | |
| (i) | (ii) | |
| A | 3.01 | 2.99 |
| B | 3.05 | 2.95 |
In a certain region of space there are only 5 molecules per cm3 on average. The temperature is 3 K. The average pressure of this very dilute gas is ______ × 10-21 atoms.
