Answer to Question #249958 in General Chemistry for clp

Question

Determine the mass in grams of 6.65 × 10²¹ atoms of barium. (The mass of one mole of barium is 137.33 g.)

Answer 1

Proportion:

A mole of barium contains 6.02×10²³ atoms.

Proportion:

1 mol - 6.02×10²³ atoms

x mol - 6.65 ×10²¹ atoms

$x= \frac{1 \times 6.65 \times 10^{21}}{6.02 \times 10^{23}} = 1.104 \times 10^{-2} \;mol \\ m = n \times M \\ m(barium) = 1.104 \times 10^{-2} \times 137.33 = 1.517 \;g$

Answer: 1.517 g