What is the density of a bar of lead that weighs 173 g and has the following dimensions: l= 2.00 cm, w = 3.00 cm, h = 1.00 in?

Explanation:

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In this case, since the density is defined as the degree of compactness of a substance, and is defined as the mass over the volume:

Given the dimensions of the bar of lead, we can compute the volume as shown below:

Thus, the density turns out:

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number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.