Answer:
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The mass in grams of 8.94×10²² formula units of CuF₂ is 15.07 g
<h3>Avogadro's hypothesis </h3>
6.02×10²³ formula units = 1 mole of CuF₂
But
1 mole of CuF₂ = 101.5 g
Thus,
6.02×10²³ formula units = 101.5 g of CuF₂
<h3>How to determine the mass of 8.94×10²² formula units of CuF₂</h3>
6.02×10²³ formula units = 101.5 g of CuF₂
Therefore,
8.94×10²² formula units = (8.94×10²² × 101.5 ) / 6.02×10²³
8.94×10²² formula units = 15.07 g of CuF₂
Thus, 8.94×10²² formula units are present in 15.07 g of CuF₂
Learn more about Avogadro's number:
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Answer:
[9x² - 2x + 8]/2x(x - 2).
Explanation:
- To do this calculation process:
We should common the denominator by multiplying the denominators of the two terms (2x)(x - 2) and dividing each denominator by the common denominator.
[2x(5x) - (x + 4)(x - 2)]/2x(x - 2)
= [10x² - (x² + 2x - 8)]/2x(x - 2)
= [10x² - x² - 2x + 8]/2x(x - 2)
= [9x² - 2x + 8]/2x(x - 2).
Answer:
The chemical symbol is always a single letter. The chemical symbol always starts with the same letter as the name of the element. The chemical symbol always begins with a capital letter. The chemical symbol can be shared by more than one element.
Explanation:
Answer:
Sample C has the highest density
Explanation:
Step 1: data given
Sample A has a mass of 224.96 grams
Sample B has a mass of 0.55632 lbs = 252.3425 grams
Sample C has a mass of 0.30648 kg = 306.48 grams
The volume is for all the sample equal
Step 2: Calculate density
We suppose the volume is 1000 mL
Density = mass / volume
Density sample A = 224.96 grams / 1000 mL = 0.22496 g/mL
Density sample B = 252.3425 grams / 1000 mL = 0.2523425 g/mL
Density sample C = 306.48 grams / 1000 mL = 0.30648 g/mL
Sample C has the highest density