Question

The mass of a single uranium atom is 4.70×10-22 grams. How many uranium atoms would there be in a sample of uranium with a volume of 278 cm3 if the density of uranium is 23.3 g/cm3?

Answer 1

Answer on Question #61938 - Chemistry - General Chemistry

Question

The mass of a single uranium atom is $4.70 \times 10^{-22}$ grams. How many uranium atoms would there be in a sample of uranium with a volume of $278~\mathrm{cm}^3$ if the density of uranium is $23.3~\mathrm{g/cm}^3$?

Solution:

The mass of a sample of uranium:

$$m = V \cdot \rho = 278 \cdot 23.3 = 6477.4 (g)$$

The number of uranium atoms:

$$N = \frac{m}{m_1} = \frac{6477.4}{4.70 \cdot 10^{-22}} = 1.38 \cdot 10^{25}$$

Answer: $N = 1.38 \cdot 10^{25}$

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