How many moles of magnesium chloride are in 5.43 x 10^24 formula units of magnesium chloride?
mole = 6.02E23 particles
5.43E24 / 6.02E23
To find the number of moles of magnesium chloride, we need to use Avogadro's number.
Step 1: Determine the formula of magnesium chloride. The chemical formula of magnesium chloride is MgCl2, which means it consists of one magnesium ion (Mg2+) and two chloride ions (Cl-).
Step 2: Determine the molar mass of magnesium chloride. The molar mass of magnesium (Mg) is approximately 24.31 g/mol, and the molar mass of chlorine (Cl) is approximately 35.45 g/mol. Since we have two chloride ions in magnesium chloride, we multiply the molar mass of chlorine by 2:
Molar mass of magnesium chloride (MgCl2) = (1 x molar mass of magnesium) + (2 x molar mass of chlorine)
= (1 x 24.31 g/mol) + (2 x 35.45 g/mol)
= 24.31 g/mol + 70.90 g/mol
= 95.21 g/mol
Step 3: Determine the number of moles using the given number of formula units. Avogadro's number states that there are 6.022 x 10^23 particles in 1 mole of a substance. We can use this conversion factor to calculate the number of moles:
Number of moles = (Number of formula units) / (Avogadro's number)
= (5.43 x 10^24 formula units) / (6.022 x 10^23 formula units/mol)
= 9.01 mol
Therefore, there are approximately 9.01 moles of magnesium chloride in 5.43 x 10^24 formula units of magnesium chloride.