FeO·TiO₂
w(Ti)=M(Ti)/M(FeO·TiO₂)
w(Ti)=47.88g/mol/151.73g/mol=0.3156 (31.56%)
Answer:
you wont be able to ask any more questions until you answer some bc you get points from answering questions but you loose points when you ask them
Explanation:
All you can conclude is that something must be burning with an orange flame.
Actually, the "something" that must be burning is the hydrogen that is produced when the sodium reacts with the water:
2Na + 2H₂O → 2NaOH + H₂ + heat
So much heat is produced that the hydrogen catches fire and some of the sodium evaporates into the flame.
The electrons in the sodium atoms get "excited" in the flame. When they drop back to a lower energy level, they emit energy in the form of an orange-yellow light.
Answer:7.229 grams of oxygen is formed by the complete reaction of 35.23 g of metallic sodium with oxygen at 130–200 °C, a process that generates sodium oxide, which in a separate stage absorbs oxygen: 4 Na + O2 → 2 Na2O. The ozone oxidizes the sodium to form sodium peroxide.
X volume= 2x2x2=8
y volume= 8x8x8=512
512/8=64 so you can fit 64
