Question

Question #7c768

Answer 1

`0.227` `"mol CO"_2`

Explanation:

We're asked to find the number of moles of `"CO"_2` in `10.0` `"g CO"_2`.

To do this, we need to find the molar mass of `"CO"_2`, which is

`overbrace((1))^"1 carbon atom"overbrace((12.011color(white)(l)"g/mol"))^" molar mass of carbon" + overbrace((2))^"2 oxygen atoms"overbrace((15.999color(white)(l)"g/mol"))^" molar mass of oxygen"`

`= color(red)(44.01color(white)(l)"g/mol"`

(the molar masses of each element can be found on a periodic table or online).

Now, we use dimensional analysis to convert from grams to moles:

`10.0cancel("g CO"_2)((1color(white)(l)"mol CO"_2)/(color(red)(44.01)cancel(color(red)("g CO"_2)))) = color(blue)(ul(0.227color(white)(l)"mol CO"_2`