# Question 40326

Jul 31, 2017

$4.42 \times {10}^{23}$ $\text{atoms H}$

#### Explanation:

I'll assume you mean sulfuric acid..

We're asked to find the number of $\text{H}$ atoms there are in $36.0$ ${\text{g H"_2"SO}}_{4}$.

To do this, let's first use the molar mass of sulfuric acid ($98.078$ $\text{g/mol}$) to find the number of moles of ${\text{H"_2"SO}}_{4}$:

36.0cancel("g H"_2"SO"_4)((1color(white)(l)"mol H"_2"SO"_4)/(98.078cancel("g H"_2"SO"_4))) = ul(0.367color(white)(l)"mol H"_2"SO"_4

Now, we can use Avogadro's number to find the number of molecules of ${\text{H"_2"SO}}_{4}$:

0.367cancel("mol H"_2"SO"_4)((6.022xx10^23color(white)(l)"molecules H"_2"SO"_4)/(1cancel("mol H"_2"SO"_4)))

= ul(2.21xx10^23color(white)(l)"molecules H"_2"SO"_4

Finally, we realize that there are $2$ atoms of hydrogen per molecule of sulfuric acid:

2.21xx10^23cancel("molecules H"_2"SO"_4)((2color(white)(l)"atoms H")/(1cancel("molecule H"_2"SO"_4)))

= color(red)(ul(4.42xx10^23color(white)(l)"atoms H"#