Question #f3e9a

Question

1016 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-01-25T22:22:19

$2$ moles.

(Reminder: $"100 gm"$ is the same thing is $"100 g"$ .)

First, let's calculate the moles of $CO_2$ that are in $"100 g"$ —to do this, we divide $"100 g"$ by the mass of $1$ mole of $CO_2$ :

$"100 g"/(CO_2 " molar mass") = "100 g"/(12.01 + 2*16.00) = 2.27$

This means there are $2.27$ moles of carbon dioxide in $"100 g"$ .

We also know that for every $1$ mole of carbon dioxide, there will be $1$ mole of carbon in it. Just look at the formula:

$CO_2$

Therefore, there are also $2.27$ moles of carbon in $"100 g"$ of carbon dioxide.

Because the question has given us $1$ significant figure, we'll just round it to $2$ moles.

Thanks so much to @Ernest Z. for telling me I misread the question! Before editing, I gave the mass of carbon instead of the moles.