What is the percent by mass of oxygen fe2o3 (formula mass= 160)?
1 answer:
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Answer:
20.(45)L or about 20.4545L
Explanation:
PV = nRT
Where:
P - pressure
V - volume
n - number of particle moles
R - a constant
T - temperature in K
We can assume the P and n (and definitely R) stay the same, so we infer that
<u>Answer:</u> 6.5 moles of silver metal is formed in the given chemical reaction. The moles of excess reagent left are 0.55 moles.
<u>Explanation:</u>
To calculate the moles of silver formed and the moles of excess reagent left after the reaction, we need to balance the equation first and need to find the limiting and excess reagent.
The balanced chemical equation is:
By Stoichiometry:
2 moles of Silver nitrate reacts with 1 mole of Zinc metal
So, 6.5 moles of silver nitrate will react with = of zinc metal
The required amount of zinc metal is less than the given amount of zinc metal, hence, it is considered as an excess reagent.
Therefore, silver nitrate is the limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 2 moles of silver metal
So, 6.5 moles of silver nitrate will produce = of silver metal.
Number of moles of excess reagent left after the completion of reaction = (3.8 - 3.25)moles = 0.55 moles
Hence, 6.5 moles of silver metal is formed in the given chemical reaction. The moles of excess reagent left are 0.55 moles.