The abundances of isotopes of hydrogen are as follows:
Isotope % Natural abundance Molar mass
$^{1} H$ $99.985$ $1$
$^{2} H$ $0.015$ $2$
Calculate the mass of a hydrogen atom.

1.00015 u

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1.00025 u

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1.00035 u

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1.00005 u

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Solution

The correct option is A 1.00015 u
The average atomic mass of hydrogen is $\frac{1 \times 99.985 + 2 \times 0.015}{100} = 1.00015 u$ .

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Similar questions

\begin{matrix} I s o t o p e & p e r N a t u r a l a b u n d a n c e & M o l a r m a s s^{1} H & 99.985 & 1^{2} H & 0.015 & 2 \end{matrix}

Calculate the average atomic mass of hydrogen using the following data

$\begin{matrix} I s o t o p e & % N a t u r a l a b u d a n c e & M o l a r m a s s^{1} H & 99.985 & 1^{2} H & 0.015 & 2 \end{matrix}$

Relative abundance of isotopes of carbon are as follows:-

The average atomic mass of carbon will be:-

_{12}^{24} M g

_{12}^{25} M g

_{12}^{26} M g

_{12}^{24} M g

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