I did the question but I need help is this right? Thanks
How many atoms of chlorine are in 19.0 grams of MgCl2?
24.3 + 2(35.5) = 95.3
19.0/95.3 x 6.022 x 1023 = 1.201 1023
1.20 x 10^23 formula units x 2 Cl atoms / formula unit = 2.40 x 10^23 Cl atoms.
looks good
To determine the number of atoms of chlorine in 19.0 grams of MgCl2, you need to use the concept of moles and Avogadro's number. Here's how you can approach it:
1. Calculate the molar mass of MgCl2:
The molar mass of magnesium chloride (MgCl2) can be calculated by adding the atomic masses of magnesium (Mg) and two chlorine (Cl) atoms:
Molar mass of MgCl2 = (1 × atomic mass of Mg) + (2 × atomic mass of Cl)
= (1 × 24.3) + (2 × 35.5)
= 24.3 + 71.0
= 95.3 g/mol
2. Determine the number of moles of MgCl2 in 19.0 grams:
To convert grams to moles, divide the given mass by the molar mass:
Number of moles = Mass (g) / Molar mass (g/mol)
Number of moles = 19.0 g / 95.3 g/mol
Number of moles = 0.1992 mol
3. Calculate the number of atoms of Cl in the given quantity of MgCl2:
Since there are 2 moles of Cl atoms in 1 mole of MgCl2, you can use the following conversion factor:
1 mole MgCl2 = 2 moles Cl
0.1992 mol MgCl2 x (2 moles Cl / 1 mole MgCl2)
= 0.3984 moles Cl
4. Finally, convert moles to the number of atoms of Cl:
To convert moles to the number of atoms, multiply the number of moles by Avogadro's number (6.022 × 10^23):
Number of atoms = Number of moles × Avogadro's number
Number of atoms = 0.3984 mol × 6.022 × 10^23/mol
Number of atoms ≈ 2.396 × 10^23 atoms
So, the correct answer is approximately 2.396 × 10^23 atoms of chlorine in 19.0 grams of MgCl2.