Question 22 (2 points)
The molar mass of Aluminum Fluoride is 83.98 grams/mol. How many grams are in 2.85 x 1023 formula units of Aluminum fluoride?
If you are unsure how to convert from particles to grams, please see the example problem linked HERE.
a
0.73 grams
b
39.7 grams
c
177.4 grams
d
1.37 grams
Step 1: Calculate the number of moles in 2.85 x 10^23 formula units of Aluminum Fluoride:
Number of formula units = 2.85 x 10^23
Molar mass of Aluminum Fluoride = 83.98 g/mol
Number of moles = (2.85 x 10^23) / Avogadro's number
Number of moles = (2.85 x 10^23) / (6.022 x 10^23)
Number of moles = 0.473 moles
Step 2: Calculate the mass of Aluminum Fluoride in grams:
Mass = Number of moles x Molar mass
Mass = 0.473 moles x 83.98 g/mol
Mass = 39.77 grams
Therefore, the answer is b) 39.7 grams.