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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.

User Miqbal
by
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2 Answers

2 votes
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

hope this helps!
User ProVega
by
7.5k points
6 votes

Answer: 3.81 grams

Step-by-step explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number
6.023* 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}=(1.20* 10^(22))/(6.023* 10^(23))=0.019moles (1L=1000ml)

Now 1 mole of
Hg atom weighs = 200.59 g

0.019 moles of
Hg atom weighs=
(200.59)/(1)* 0.019=3.81g

Thus mass of sample of mercury is 3.81 grams

User Syntagma
by
8.0k points
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