what is the mass in grams?
a) 3.011 x 10^23 atoms F
b)1.50 x 10^23 atoms Mg
c)4.50 x 10^12 atoms Cl
d)8.42 x 10^18 atoms Br
e) 25 atoms w
f) 1 atom Au
can you please explain a and b to me then i'll come back later and see if i did the rest right? Thanks in advance
it needs to be in scientific notation i think.
answered above.
To find the mass in grams of a given number of atoms, you'll need to use the concept of atomic mass and Avogadro's number. Here's how you can calculate the mass for options (a) and (b):
(a) 3.011 x 10^23 atoms F:
1. Locate the atomic mass of fluorine (F) on the periodic table, which is approximately 19.00 grams.
2. Multiply the atomic mass by the given number of atoms:
19.00 g/mol * (3.011 x 10^23 atoms) = 5.72 x 10^24 grams
So, the mass is approximately 5.72 x 10^24 grams.
(b) 1.50 x 10^23 atoms Mg:
1. Find the atomic mass of magnesium (Mg) on the periodic table, which is approximately 24.31 grams.
2. Multiply the atomic mass by the given number of atoms:
24.31 g/mol * (1.50 x 10^23 atoms) = 3.65 x 10^24 grams
The mass is approximately 3.65 x 10^24 grams.
I hope this helps! Let me know if you have any further questions.
To find the mass in grams, we need to use the concept of molar mass and Avogadro's number.
First, we need to convert the number of atoms given into moles by dividing the given number by Avogadro's number (6.022 x 10^23).
For option a) 3.011 x 10^23 atoms F:
To find the mass in grams, we will use the molar mass of fluorine (F), which is approximately 19.0 grams/mole.
1 mole (F) = 6.022 x 10^23 atoms
1 mole (F) = 19.0 grams
So, we can set up a proportion:
(3.011 x 10^23 atoms / 6.022 x 10^23 atoms) = (x grams / 19.0 grams)
Cross-multiplying and solving for x, the mass in grams is approximately:
x grams ≈ (3.011 x 10^23 atoms / 6.022 x 10^23 atoms) * 19.0 grams
x grams ≈ 9.5 grams
Therefore, option a) has a mass of approximately 9.5 grams.
For option b) 1.50 x 10^23 atoms Mg:
Similar to the previous calculation, we need to use the molar mass of magnesium (Mg), which is approximately 24.3 grams/mole.
1 mole (Mg) = 6.022 x 10^23 atoms
1 mole (Mg) = 24.3 grams
Setting up the proportion:
(1.50 x 10^23 atoms / 6.022 x 10^23 atoms) = (x grams / 24.3 grams)
Cross-multiplying and solving for x, the mass in grams is approximately:
x grams ≈ (1.50 x 10^23 atoms / 6.022 x 10^23 atoms) * 24.3 grams
x grams ≈ 6.1 grams
Therefore, option b) has a mass of approximately 6.1 grams.
Please let me know if you need assistance with the other options as well.