Based on the calculations, the mass of Aluminum in 4.85 × 10²² atoms is equal to 2.1762 grams.
<h3>How to calculate the mass of Aluminum?</h3>
In order to determine the mass of Aluminum, we would calculate the number of atoms in 1 mole of an Aluminum atom in accordance with Avogadro's constant.
1 mole of Aluminum atom = 6.02 × 10²³ molecules
X moles of Aluminum atom = 4.85 × 10²² molecules
Cross-multiplying, we have:
X = 4.85 × 10²²/6.02 × 10²³
X = 0.0806 moles.
Mass = Molar mass × Number of moles
Mass = 27 × 0.0806
Mass = 2.1762 grams.
Read more on moles here: brainly.com/question/3173452
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<span>If two fluorine atoms bonded with each other what kind of bond would be involved?
A. ionic
B. valence
C. covalent
D. non-metallic
C. covalent
</span>
Answer:
true
Explanation:
I think it is true but im uncertain
Initial pressure of the gas = 65.3 kPa
Initial volume of the gas = 654 cm³
Initial temperature of the gas = 6⁰C = 273 + 6 = 279 K
Final pressure of the gas = 108.7 kPa
Final temperature of the gas = 4⁰C = 273 + 4 = 277 K
Using the combined gas law for ideal gases:
P₁V₁/T₁ = P₂V₂/T₂
where P₁, V₁ and T₁ are the pressure, volume and temperature for the initial state and P₂, V₂ and T₂ are the pressure, volume and temperature for the final state.
Plugging the given data into the combined gas law we have,
(65.3 kPa x 654 cm³) / (279 K) = (108.7 kPa x V₂)/(277 K)
V₂ = (65.3 kPa x 654 cm³ x 277 K) / (279 K x 108.7 kPa)
V₂ = 390.1 cm³