Answer : The molecular weight of this compound is 891.10 g/mol
Explanation : Given,
Mass of compound = 12.70 g
Mass of ethanol = 216.5 g
Formula used :
where,
= change in freezing point
= temperature of pure ethanol = 
= temperature of solution = 
= freezing point constant of ethanol = 
i = van't hoff factor = 1 (for non-electrolyte)
m = molality
Now put all the given values in this formula, we get
Therefore, the molecular weight of this compound is 891.10 g/mol
The decomposition of Al2O3 to form pure aluminum (Al) along with the release of oxygen (O2) gas can be represented by the following chemical reaction:
2Al2O3 → 4Al + 3O2
Based on the reaction stoichiometry:
2 moles of aluminum oxide decomposes to form 4 moles of pure aluminum
Therefore, if 29.0 moles of aluminum is recovered, then the moles of aluminum oxide required will be:
= 29.0 moles Al * 2 moles Al2O3/4 moles Al
= 14.5 moles of Al2O3
So,
These species react stoichiometrically. Thus, we can say, for example, that 1 mol A is stoichiometrically equivalent to 1 mol B in this reaction. I will say A = B.
A = B
A = C
A = D
B = C
B = D
C = D
As you can see, there are more than 4 distinct mole ratios for this reaction. Thus, the statement is false.
Humans get<span> the </span>nitrogen<span> they need by eating vegetebles or other meat that contain </span>nitrogen<span>. hope it helps :)</span>
Answer:
125g
Explanation:
you simply add the masses together
