What is the mass, in grams, of a sample of 1.20 × 1022 atoms of mercury (Hg)? Show your work or explain the steps that you used to determine your answer.

Atomic mass Hg = 200.59 u.m.a

200.59 g --------------- 6.02x10²³ atoms
( mass Hg ) ----------- 1.20 x10²² atoms

mass Hg = ( 1.20x10²² ) x 200.59 / 6.02x10²³

mass Hg = 2.407x10²⁴ / 6.02x10²³

= 3.998 g of Hg

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kobenhavn kobenhavn · Answer 2 · 2019-06-30T08:29:14-04:00

Answer: 3.81 grams

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number \(6.023\times 10^{23}\) of particles.

To calculate the moles, we use the equation:

\(\text{Number of moles}=\frac{\text{Given atoms}}{\text {Avogadro's number}}\)

\(\text{Number of moles}=\frac{1.20\times 10^{22}}{6.023\times 10^{23}}=0.019moles\) (1L=1000ml)

Now 1 mole of \(Hg\) atom weighs = 200.59 g

0.019 moles of \(Hg\) atom weighs= \(\frac{200.59}{1}\times 0.019=3.81g\)

Thus mass of sample of mercury is 3.81 grams