Answer:
1,7Kg of
is produced
Explanation:
<em>Balanced chemical reaction</em>
To find the mass of
produced in a reaction, we need to start by identifying that chemical reaction and balancing it.
The question give us the reactants and the products, do we know:
+
⇒
+ ![H_{2} O](https://tex.z-dn.net/?f=H_%7B2%7D%20O)
Counting C, H and O in reactants and products; and balancing them with stoichiometric coefficients, we have that the balanced chemical equation is:
2
+ 160
⇒ 114
+ 110 ![H_{2} O](https://tex.z-dn.net/?f=H_%7B2%7D%20O)
<em>Stoichiometry</em>
The question says us that 1.2 Kg of fat (
) react.
To find the amount of
we need to find the moles of
. The way to do it, is using the molar mass:
Taking the molar mass of each element in the periodic table, multiplying by the subscript and adding all the partial values:
![(12.0107)*57+(1.00794)*110+(15.9994)*6= 891.48 \frac{g}{mol}](https://tex.z-dn.net/?f=%2812.0107%29%2A57%2B%281.00794%29%2A110%2B%2815.9994%29%2A6%3D%20891.48%20%5Cfrac%7Bg%7D%7Bmol%7D)
The moles of
that react are:
![C_{57}H_{110}O_{6}](https://tex.z-dn.net/?f=C_%7B57%7DH_%7B110%7DO_%7B6%7D)
The balanced chemical reaction tell us that each 2 moles of
that react, produce 110 moles of
. It means that:
1.6826 mol
![* \frac{110 mol H_{2}O}{2 mol C_{57}H_{110}O_{6}}](https://tex.z-dn.net/?f=%2A%20%5Cfrac%7B110%20mol%20H_%7B2%7DO%7D%7B2%20mol%20C_%7B57%7DH_%7B110%7DO_%7B6%7D%7D)
mol ![H_{2} O](https://tex.z-dn.net/?f=H_%7B2%7D%20O)
Finally, using the molar mass of
, we can find its mass:
92.543 mol ![H_{2} O](https://tex.z-dn.net/?f=H_%7B2%7D%20O)
=1665.7 g
With two sig figs, the mass:
1665.7g
≅ 1.7 Kg