Number of tin atoms

Tin has a density of 7.31 g/cm^3. How many tin atoms are in a block of tin that is 5.48 inches wide by 3.02 inches high by 14.41 inches long?

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First find the volume of the block of tin. To do this first convert inches to cm by multiplying each dimension by 2.54 since there are 2.54 cm in one inch.

2.54* 5.48 =13.92 cm

2.54 * 3.02 = 7.67 cm

2.54 * 14.41 = 36.6 cm

V = lwh = 13.92 * 7.67 * 36.6 =3907.7 cc

Since density is 7.31 g/1 cc, you have 7.31g/cc * 3907.7 cc =28565.2 grams of tin.

The atomic mass of tin is 118.7 g/mole

So find number of moles of tin

28565.2g/118.7 g per mole = 240.65 moles of tin.

One mole contains Avogadro's number of atoms, so multiply moles times Avogadro's number for the answer.

6.02 x 10^23 * 2.4065 * 10^2 = 1.45 * 10^26 atoms in the block.

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