Answer:
13.5 g
Explanation:
This question is solved easily if we remember that the number of moles is obtained by dividing the mass into the atomic weight or molar mass depending if we are referring to elements or molecules.
Therefore, the mass of aluminum in the reaction will the 0.050 mol Al times the atomic weight of aluminum.
number of moles = n = mass of Al / Atomic Weight Al
⇒ mass Al = n x Atomic Weight Al = 0.050 mol x 27 g mol⁻¹
= 13.5 g
We have three significant figures in 0.050 and therefore we should have three significant figures in our answer.
Mass of aluminum that participated in the chemical reaction is 1.35 grams.
Number of Moles:
Number of moles is defined as the ratio of given mass to the molar mass.
Given:
Moles of Aluminum = 0.050 moles
To find:
Mass of Aluminum=?
As we know, Molar mass of Aluminum = 27g/mol
On substituting the values:
[tex]\text{Number of Moles}=\frac{\text{Given mass}}{\text{Molar mass}} \\\\ \text{Given mass}= \text{Number of Moles}*\text{Molar mass}\\\\ \text{Given mass}= 0.050*27\\\\ \text{Given mass}=1.35\text{ grams}[/tex]
Thus, the mass of aluminum that participated in the chemical reaction is 1.35 grams.
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