A sample of Ba3(PO4)2 contains 14.5 g of O. How many g of Ba are in the sample?
To determine the grams of Ba in the sample, we can use the molar ratio between Ba and O in the compound Ba3(PO4)2.
The atomic mass of O is 16 g/mol, and since there are 14.5 g of O in the sample, we can calculate the number of moles of O by dividing the mass by the atomic mass:
Number of moles of O = mass of O / atomic mass of O
= 14.5 g / 16 g/mol
= 0.90625 mol
Next, we can use the balanced chemical equation of Ba3(PO4)2 to determine the molar ratio between Ba and O. From the formula, we see that Ba3(PO4)2 contains a ratio of 3 moles of Ba for every 8 moles of O.
Using this ratio, we can calculate the number of moles of Ba in the sample:
Number of moles of Ba = (3/8) * Number of moles of O
= (3/8) * 0.90625 mol
= 0.33984375 mol
Finally, we can determine the mass of Ba in grams by multiplying the number of moles of Ba by the atomic mass of Ba, which is 137.33 g/mol:
Mass of Ba = number of moles of Ba * atomic mass of Ba
= 0.33984375 mol * 137.33 g/mol
= 46.654296875 g
Therefore, there are approximately 46.65 g of Ba in the sample of Ba3(PO4)2.
14.5 g O/16 = mols O.
1/8 mols O = mols Ba3(PO4)2
3x that = mols Ba
g Ba = mols Ba x atomic mass Ba