Determine the number of moles of compound in each of the following samples.?
4.50g h2o
471.6g ba(oh)2
129.68g fe3(po4)2

For the answer to the question above, we have to use this formula
moles equal mass divided by the molar mass 

a) 4.50 g divided by the molar mass of water 
molar mass of water = 2x1.0 + 1x16.0 = 18 
4.50 g / 18.0 g per mole = 0.25 moles 

b) 471.6 g / Molar mass of Ba(OH)2 = moles 

c) 129.68 g / molar mass of Fe3(PO4)2 = moles 

atoms of P in Mg3(PO4)2 
2 atoms of P in each molecule of Mg3(PO4)2 
247 g / molar mass of Mg3(PO4)2 = moles 
moles of Mg3(PO4)2 x 6.022x10^23 = molecules of Mg3(PO4)2

I hope my answers gave you clarity on your question.

Explanation:

To calculate the number of moles, we use the equation:

   ......(1)

For 1: 4.50 g of water

Given mass of water = 4.50 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

Hence, the moles of given amount of water is 0.25 moles.

For 2: 471.6 g of barium hydroxide

Given mass of barium hydroxide = 471.6 g

Molar mass of barium hydroxide = 171.34 g/mol

Putting values in equation 1, we get:

Hence, the moles of given amount of barium hydroxide is 2.75 moles.

For 3: 129.68 g of iron phosphate

Given mass of iron phosphate = 129.68 g

Molar mass of iron phosphate = 150.82 g/mol

Putting values in equation 1, we get:

Hence, the moles of given amount of iron phosphate is 0.86 moles.

I’m pretty sure it’s false i’m not sure

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