A sample of AlF3 contains 3.0 x 10^24 F- ions. The number of formula units in this sample is:
Correct answer: D. 1 x 10^24
- A. 9.0 x 10^24
- B. 0.75 x 10^24
- C. 3.0 x 10^24
- D. 1 x 10^24
Explanation
The formula of AlF3 suggests that there are three fluoride ions (F-) for each aluminum ion (Al3+). Given that there are 3.0 x 1024 F- ions, we can calculate the number of formula units of AlF3 as follows: Number of formula units = (Number of F- ions) / (Number of F- ions per formula unit of AlF3) Number of formula units = (3.0 x 10^24) / 3 Number of formula units = 1.0 x 10^24 So, there are 1.0 x 1024 formula units of AlF3 in the given sample. Hence option D is correct.
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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