Dinitrogen pentoxide is used in the preparation of explosives. If 7.93 mol of
1 answer:
The volume of O₂ produced: 84.6 L
<h3>Further explanation</h3>Given
7.93 mol of dinitrogen pentoxide
T = 48 + 273 = 321 K
P = 125 kPa = 1,23365 atm
Required
Volume of O₂
Solution
Decomposition reaction of dinitrogen pentoxide
2N₂O₅(g)→4NO₂(g)+O₂ (g)
From the equation, mol ratio N₂O₅ : O₂ = 2 : 1, so mol O₂ :
= 0.5 x mol N₂O₅
= 0.5 x 7.93
= 3.965 moles
The volume of O₂ :
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Answer:
10.60 grams of silane gas are formed.
Explanation:
From the reaction:
Mg₂Si(s) + 4H₂O(l) → 2Mg(OH)₂(aq) + SiH₄(g)
We know that the limiting reactant is Mg₂Si, so to find the mass of SiH₄ formed we need to calculate the number of moles of Mg₂Si:
Where:
m: is the mass of Mg₂Si = 25.0 g
M: is the molar mass of Mg₂Si = 76.69 g/mol
Now, the stoichiometric relation between Mg₂Si and SiH₄ is 1:1 so:
Finally, the mass of SiH₄ is:
Therefore, 10.60 grams of silane gas are formed.
I hope it helps you!
Answer:
Here's what I get
Explanation:
The fatty acids form ester C-O bonds with the OH groups of glycerol and the phosphoric acid forms phosphate P-O bonds.
The phosphate also forms P-O ester linkages with the OH groups in other alcohols such as choline.
The structure below shows the phospholipid with two saturated C₈ fatty acids and the phosphate group.
