<span>The atomic weight of 13C should be pretty close to 13.0. (If you have the exact mass, use it in the problem.) So,
9.00 g / 13.0 g/mol = 0.692 moles
Therefore, the answer should be 0.692 moles are in 9.00 g of 13C.</span>
Answer:
26.3 moles of O₂ are needed to react completely with 35.0 mol of FeCl₃
Explanation:
To determine the number of moles of O₂ that are needed to react completely with 35.0 mol of FeCl₃, it is possible to use the reaction stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), and rule of three as follows: if 4 moles of FeCl₃ react with 3 moles of O₂, 35 moles of FeCl₃ with how many moles of O₂ will it react?
![molesofO_{2} =\frac{35 moles of FeCl_{3}*3 moles of O_{2} }{4 moles of FeCl_{3}}](https://tex.z-dn.net/?f=molesofO_%7B2%7D%20%3D%5Cfrac%7B35%20moles%20of%20FeCl_%7B3%7D%2A3%20moles%20of%20O_%7B2%7D%20%20%7D%7B4%20moles%20of%20FeCl_%7B3%7D%7D)
moles of O₂= 26.25 ≅ 26.3
<u><em>26.3 moles of O₂ are needed to react completely with 35.0 mol of FeCl₃</em></u>
Answer:
Law of Conservation of Energy
Explanation:
Pretty sure it's the Precambrian.