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.
2 answers:
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 of particles.
To calculate the moles, we use the equation:
(1L=1000ml)
Now 1 mole of atom weighs = 200.59 g
0.019 moles of atom weighs=
Thus mass of sample of mercury is 3.81 grams
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!
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