Atomic and Molecular Mass

Specific volume of a cylindrical virus particle whose radius and length are $7 \mathrm{\AA }$ and $10 \mathrm{\AA }$ respectively, is  $6.02\times {10}^{-2}\mathrm{cc}/\mathrm{g}$. If  ${\mathrm{N}}_{\mathrm{A}}=6.02\times {10}^{23}$, find the molecular weight of the virus:

A compound, on analysis, gave the following percentage composition :
$\mathrm{Na}=14.31\%,\mathrm{S}=9.97\%,\mathrm{H}=6.22\%,\mathrm{O}=69.5\%$ 

What would be the molecular formula of the compound assuming that all the hydrogen in the compound is reset in combination with oxygen as water of crystallisation. Molecular weight of the compound is $322$.

Total number of atoms in $18 \mathrm{amu}$ of ${\mathrm{H}}_2\mathrm{O}$ is

If the table of atomic masses were established with the oxygen atom and assigned value of 200, then the mass of carbon atom would be, approximately:

An element 'A' have 3 isotopes A²⁴,A²⁸ & A³⁰,if percentage abundance of A²⁴ is 50% then calculate percentage abundance of A²⁸ and A³⁰
(Given : average atomic mass = 26.8)

Calculate the molar mass of glucose

An element $x$ has $3$ isotopes and its average atomic mass is $24.5$. If the percentage isotopic abundance of ${\mathrm{x}}^{24}$ is$40\%$,the percentage abundances of $x^{25}$ and $x^{26}$ are respectively

Which atom was originally used as a reference element for defining the atomic masses of other atoms.

The relative atomic mass of nitrogen assuming oxygen as the reference element is

Define amu assuming oxygen as the reference element.

Calculate the atomic mass of nitrogen assuming oxygen as the reference element.

Which element is used as a reference element in the present system of atomic masses?

What is the difference between mass number and relative atomic mass?

An element X has the following isotopic composition:
${}^{200}\mathrm{X}:90\raisebox{1ex}{$ \mathrm{o}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{o}$}\right.$ ,  ${}^{199}\mathrm{X}:8.0 \raisebox{1ex}{$\mathrm{o}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{o}$}\right.$ ,   ${}^{202}\mathrm{X}:2 \raisebox{1ex}{$\mathrm{o}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{o}$}\right.$
The weighted average atomic mass of the naturally occurring element X is close to

The gram atomic mass of zinc is:

An element X has the following isotopic composition:
${}^{200}\mathrm{X}:90\raisebox{1ex}{$ \mathrm{o}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{o}$}\right.$ ,  ${}^{199}\mathrm{X}:8.0 \raisebox{1ex}{$\mathrm{o}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{o}$}\right.$ ,   ${}^{202}\mathrm{X}:2 \raisebox{1ex}{$\mathrm{o}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{o}$}\right.$
The weighted average atomic mass of the naturally occurring element X is close to

The average atomic mass of magnesium is $24.31 \mathrm{amu}$. This magnesium is composed of $79$mole $\%$ of  ${}^{24}\mathrm{Mg}$ and remaining $21$ mole $\%$ of  ${}^{25}\mathrm{Mg}$ and ${}^{26}\mathrm{Mg}$. Calculate mole $\%$ of ${}^{26}\mathrm{Mg}$.

Average atomic mass of $\mathrm{Mg}$ is approximately equal to. (Given that percentage abudance of ${{12}^{\mathrm{Mg}}}^{24}$, ${{12}^{\mathrm{Mg}}}^{25}$ and ${{12}^{\mathrm{Mg}}}^{26}$ are $79\%, 10\% \mathrm{and} 11\%$, respectively)