By definition,

density $=\frac{\text{m}\text{a}\text{s}\text{s}}{\text{v}\text{o}\text{l}\text{u}\text{m}\text{e}}$

Typical units of density are $\frac{g}{m}L$ or $\frac{g}{c}{m}^3.$

$1mL=1c{m}^3$

Most elements occur naturally as a mix of different isotopes. An

element's atomic mass is the weighted average of the isotope masses

In other words, it is an average that takes into account the percentage

of each isotope. For example, the two naturally occurring isotopes of

boron are given here.

The atomic mass of boron is calculated as follows:

$(10\mathrm{.}00\mathrm{.}100)+(11\mathrm{.}00\mathrm{.}801)-10\mathrm{.}8u$

Because the heavier isotope is more abundant, the atomic mass is

closer to $11u$ than it is to $10u.$

Part A

The density of iron is $7\mathrm{.}87\frac{g}{m}L.$ What is the mass of a $5\mathrm{.}00cm4\mathrm{.}00cm1\mathrm{.}00cm$ block of iron?

Express your answer to three significant figures and include the appropriate units.

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mass $=$

Part A

What is the atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances?

Express your answer to three significant figures and include the appropriate units.

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Part B

What is the atomic mass of the element that consists of the following isotopes in the indicated natural abundances?

Express your answer to three significant figures and include the appropriate units.

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