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 177.4 grams c 1.37 grams d 39.7 grams
To convert from particles to grams, you can use the following steps:
1. Calculate the number of moles in 2.85 x 10^23 formula units of Aluminum Fluoride:
2.85 x 10^23 formula units / 6.022 x 10^23 formula units/mol = 0.474 moles
2. Convert moles to grams using the molar mass of Aluminum Fluoride (83.98 g/mol):
0.474 moles x 83.98 g/mol = 39.7 grams
Therefore, the answer is d) 39.7 grams