Question

Question #7baa6

Answer 1

Well, we know that `1*mol` of Ideal gas at `"STP"` occupies `22.4*L`...

Explanation:

And thus if we assume that carbon dioxide behaves ideally (which is a reasonable assumption, then we have `(224*L)/(22.4*L*mol^-1)`, i.e. a `10*mol` quantity of `CO_2`.....And I think you can see why they specified this particular volume.

And thus there is a `10*mol` quantity of carbon, i.e. `10*molxx12.00*g*mol^-1=120.0*g`........

And likewise there is `20*molxx15.999*g*mol^-1=320.0*g`........with respect to `"oxygen"`.

And you should not have to remember the atomic masses (tho you will soon retain the common masses) because you should be provided with a Periodic Table.