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hydrogen is found primarily as two isotopes in nature: (1.0078u) and (2.0140u). Caluclate the percentage abundance of each isotope based on hydrogens average atomic mass

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Pyromorphiteid
hydrogens average atomic mass = 1,01u

x = isotope about mass (1.0078u)
y = isotope about mass (2.0140u)

x + y = 100%
so:
x = 100% - y

[tex]hydrogens ~average~atomic~mass=\frac{(1.0078\cdot x)+(2.0140\cdot y)}{100}\\ 1.01=\frac{(1.0078\cdot (100-y))+(2.0140y)}{100}||\cdot 100\\ 101=100.78-1.0078y+2.0140\\ 101-100.78=1.0062y\\ 0,22=1.0062y||:1.0062\\ 0.219\%=y\\\\ x=100\%-y\\ x=100\%-0.219\%\\ x=99.781\%\\\\ [/tex]

answer:
[tex]x=99.781\%\\ y=0.219\%[/tex]

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