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marshall27 [118]
3 years ago
7

How many atoms are in a 2.70 cm × 2.70 cm × 2.70 cm cube of aluminum?

Physics
1 answer:
Bess [88]3 years ago
4 0

First, we calculate for the total volume of aluminum. The volume of a cube is:

V = s * s * s = s^3

V = (2.70 cm)^3

V = 19.683 cm^3

Assuming atmospheric temperature, the density of aluminum is about 2.70 g / cm^3. Therefore the equivalent mass of aluminum is:

m = 19.683 cm^3 * 2.70 g / cm^3

m = 53.1441 g

The molar mass of aluminum is 27 g / mol. Therefore the number of moles is:

n = 53.1441 g / (27 g / mol)

n = 1.9683 mol

Given the number of moles, we can calculate for the number of atoms using Avogadro’s number.

atoms = 1.9683 mol * (6.022 * 10^23 atoms / mol)

<span>atoms = 11.85 * 10^23 atoms               (ANSWER)</span>

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           u - 2.5 g = u - 4.5 g + 3

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3 years ago
Click the links to open the resources below. These resources will help you complete the assignment. Once you have created your f
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Explanation:

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Yes, yes, we know all of that.  It certainly took you long enough to
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If
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Fudgin [204]

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3 years ago
If a person is standing erect and flexes the trunk on the hip, the center of mass will move __________ and the line of gravity m
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anterior

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hope this helps any further query can be asked in comment section.

8 0
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