# Question 943f0

Aug 14, 2016

$\text{6.4 g}$

#### Explanation:

The Law of Definite Proportions states that a given compound will always have the same mass ratios between its constituent elements.

Simply put, its constituent elements will always combine in the same mass ratio to form said compound.

In your case, you know that the compound is carbon monoxide, $\text{CO}$.

You also know that a given sample of this compound contains $\text{2.4 g}$ of carbon and $\text{3.2 g}$ of oxygen. This is the mass ratio in which the elements combined to form a mass of

$\text{2.4 g " + " 3.2 g" = "5.6 g}$

of carbon monoxide. The mass ratio that exists between the elements takes the form

"mass of C"/"mass of O" = (2.4 color(red)(cancel(color(black)("g"))))/(3.2color(red)(cancel(color(black)("g")))) = 3/4

This means that when any mass of carbon monoxide is formed, the mass of carbon and the mass of oxygen must be in a $\frac{3}{4}$ ratio in order for the Law of Definite Proportions to hold true.

Simply put, for every $\text{3 g}$ of carbon present in a sample of carbon monoxide, you also have $\text{4 g}$ of oxygen.

You can thus say that $\text{4.8 g}$ of carbon will combine with

4.8 color(red)(cancel(color(black)("g C"))) * "4 g O"/(3color(red)(cancel(color(black)("g C")))) = color(green)(|bar(ul(color(white)(a/a)color(black)("6.4 g O")color(white)(a/a)|)))#