0.500 mol of Ca(IO3)2 contains ------ mol of iodine, I; to supply this much iodine,----- g of calcium iodate are needed. [Iodised salt contains a trace amount of calcium iodate, Ca(IO3)2, to help prevent a thyroid condition called goitre.]
0.500 mole Ca(IO3)2 x (2 moles I/1 mole Ca(IO3)2).
Now convert moles to grams. g I = moles I x atomic mass I.
Well, let me calculate that for you. Considering the molar mass of Ca(IO3)2 is 389.88 g/mol, we can determine the number of moles of iodine present by multiplying the molar mass of iodine (126.90 g/mol) by the number of iodine atoms in one molecule of Ca(IO3)2, which is 2. Therefore, 0.500 mol of Ca(IO3)2 contains 2 * 0.500 = 1 mol of iodine.
To find the mass of calcium iodate needed, we can multiply the molar mass of Ca(IO3)2 by the number of moles of calcium iodate required, which is 1 mol. So, the mass of calcium iodate needed is 389.88 g/mol.
Now, I wouldn't recommend adding calcium iodate to your favorite dish as a seasoning. It's better used to prevent goitre!
To find the number of moles of iodine (I) in 0.500 mol of Ca(IO3)2, we need to consider the ratio of iodine to calcium iodate.
The chemical formula for calcium iodate is Ca(IO3)2, which indicates that there are 2 iodine atoms (I) in each formula unit.
Step 1: Calculate the number of moles of iodine (I):
Number of moles of iodine (I) = 0.500 mol × 2 mol I/mol Ca(IO3)2
Number of moles of iodine (I) = 1.000 mol I
Therefore, 0.500 mol of Ca(IO3)2 contains 1.000 mol of iodine (I).
To determine the grams of calcium iodate (Ca(IO3)2) needed to supply this amount of iodine, we need to know the molar mass of calcium iodate.
Step 2: Calculate the molar mass of calcium iodate (Ca(IO3)2):
Calcium (Ca) atomic mass = 40.08 g/mol
Iodine (I) atomic mass = 126.90 g/mol
Oxygen (O) atomic mass = 16.00 g/mol
Molar mass of Ca(IO3)2 = (Ca atomic mass × 1) + (I atomic mass × 2) + (O atomic mass × 6)
Molar mass of Ca(IO3)2 = (40.08 g/mol × 1) + (126.90 g/mol × 2) + (16.00 g/mol × 6)
Molar mass of Ca(IO3)2 = 40.08 g/mol + 253.80 g/mol + 96.00 g/mol
Molar mass of Ca(IO3)2 = 389.88 g/mol
Step 3: Calculate the grams of calcium iodate (Ca(IO3)2) needed:
Grams of Ca(IO3)2 = Number of moles of iodine (I) × Molar mass of Ca(IO3)2
Grams of Ca(IO3)2 = 1.000 mol × 389.88 g/mol
Grams of Ca(IO3)2 = 389.88 g
Therefore, to supply the iodine in 0.500 mol of Ca(IO3)2, approximately 389.88 g of calcium iodate are needed.
To determine the number of moles of iodine (I) in 0.500 mol of Ca(IO3)2, we need to consider the ratio of iodine atoms to calcium iodate.
The chemical formula of calcium iodate, Ca(IO3)2, tells us that for every 1 mol of calcium iodate, we have 2 moles of iodine atoms.
Therefore, since we have 0.500 mol of calcium iodate (Ca(IO3)2), we can calculate the number of moles of iodine (I) as follows:
Number of moles of iodine (I) = 0.500 mol of calcium iodate (Ca(IO3)2) x 2 moles of iodine / 1 mole of calcium iodate
Number of moles of iodine (I) = 0.500 mol x 2 moles / 1 mole = 1.000 mol
Therefore, 0.500 mol of Ca(IO3)2 contains 1.000 mol of iodine.
Now, to determine the mass of calcium iodate (Ca(IO3)2) needed to supply this much iodine, we need to use the molar mass of calcium iodate.
The molar mass of calcium iodate (Ca(IO3)2) can be calculated by summing the atomic masses of its constituent elements.
Molar mass of calcium iodate (Ca(IO3)2) = (atomic mass of calcium (Ca)) + 2 * (atomic mass of iodine (I)) + 6 * (atomic mass of oxygen (O))
Using the atomic masses from the periodic table, we can calculate the molar mass of calcium iodate as follows:
Molar mass of calcium iodate (Ca(IO3)2) = (40.08 g/mol) + 2 * (126.90 g/mol) + 6 * (16.00 g/mol)
Molar mass of calcium iodate (Ca(IO3)2) = 40.08 g/mol + 253.80 g/mol + 96.00 g/mol = 389.88 g/mol
Therefore, to supply 1.000 mol of iodine, we would need:
Mass of calcium iodate (Ca(IO3)2) = 1.000 mol of iodine x (389.88 g/mol) / 1 mol of iodine
Mass of calcium iodate (Ca(IO3)2) = 389.88 g
So, to supply this much iodine, 389.88 g of calcium iodate (Ca(IO3)2) would be needed.