What is the mass in grams of the following:
a) 3.011x10 to the 12th power atoms F
b)1.50x10 to the 23 power atoms Mg
1 mol F has a mass of 19.00 g and there are 6.02 x 10^23 atoms in that mass. Therefore, 19.00 x (3.011 x 10^12/6.02 x 10^23)= ??
The second one is done the same way. Look up the mass of Mg in the periodic table. I think it is 24.32 g/mol.
Thank you Dr. Bob
10 to the power of 12
To find the mass in grams, you need to use the concept of molar mass and Avogadro's number. Here are the step-by-step explanations on how to calculate the mass in grams for both scenarios.
a) 3.011x10^12 atoms of F:
Step 1: Determine the atomic mass of fluorine (F) from the periodic table, which is approximately 19 g/mol.
Step 2: Multiply the atomic mass by Avogadro's number, which is 6.022 x 10^23 atoms/mol, to find the molar mass:
19 g/mol x (1 mol / 6.022x10^23 atoms) = 3.16 x 10^-23 g/atom
Step 3: Calculate the mass by multiplying the molar mass by the given number of atoms:
3.16 x 10^-23 g/atom x 3.011 x 10^12 atoms = 9.5 grams
Therefore, the mass of 3.011x10^12 atoms of F is approximately 9.5 grams.
b) 1.50x10^23 atoms of Mg:
Step 1: Find the atomic mass of magnesium (Mg) on the periodic table, which is approximately 24.3 g/mol.
Step 2: Multiply the atomic mass by Avogadro's number (6.022 x 10^23 atoms/mol) to get the molar mass:
24.3 g/mol x (1 mol / 6.022x10^23 atoms) = 4.03 x 10^-23 g/atom
Step 3: Calculate the mass by multiplying the molar mass by the given number of atoms:
4.03 x 10^-23 g/atom x 1.50 x 10^23 atoms = 6.04 grams
Therefore, the mass of 1.50x10^23 atoms of Mg is approximately 6.04 grams.