Question b0d55

Jul 6, 2017

Here's what I got.

Explanation:

For starters, you need to have a balanced chemical equation to go by here. As you can see, carbon will react with oxygen gas in a $1 : 1$ mole ratio to produce carbon dioxide in a $1 : 1$ mole ratio.

This means that the number of moles of carbon that take part in the reaction will be equal to the number of moles of carbon dioxide produced by the reaction.

Now, you know that the reaction produced $\text{50 g}$ of carbon dioxide, so use the compound's molar mass to convert this to moles

50 color(red)(cancel(color(black)("g"))) * "1 mole CO"_2/(44.01color(red)(cancel(color(black)("g")))) = "1.136 moles CO"_2#

You can thus say that the reaction produced $1.136$ moles of carbon dioxide, which implies that it must have consumed $1.136$ moles of carbon.

To convert this to grams, use the element's molar mass

$1.136 \textcolor{red}{\cancel{\textcolor{b l a c k}{\text{moles C"))) * "12.01 g"/(1color(red)(cancel(color(black)("mole C")))) = color(darkgreen)(ul(color(black)("14 g}}}}$

I'll leave the answer rounded to two sig figs, but keep in mind that you only have one significant figure for the mass of carbon dioxide.