3. calculate the following quantities a. mass in grams of 1.223 mol Fe2(SO4)3 b.

Question

3. calculate the following quantities

a. mass in grams of 1.223 mol Fe2(SO4)3

b. moles of NH4+ ions in 6.995 g of (NH4)2CO3

c. mass in grams of 7.70 x 10^20 molecules of aspirin , C8H10N4O2

d. molar mass of diazepam if 0.05570 mol has a mass of 15.85 g

4.determine the empirical and molecular formulas

a. ibuprofen contains 75.69% C, 8.80% H, and 15.51% O mass. It has a molar mass of 206 g/mol.

b. Cadaverine contains 58.55% C, 13.81% H, and 27.40% N by mass, and has a molar mass of 102 g/mol.

c. Adrenaline contains 59.0% C, 7.1% H, 26.2% O, and 7.7% and has a molar mass of about 180 g/mol.

5. Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of molecules of water are included in the solid structure. The formula for the Epsom salts can be written as MgSO4 * XH2O where x indicates the number of moles of H2O per mole of MgSO4. When 5.061g of this hydrate is heated to 250 degree c, all of the water hydration is lost, leavng 2.472g of MgSO4. What is the value of x?

Explanation / Answer

3. calculate the following quantities

a. mass in grams of 1.223 mol Fe2(SO4)3

MW Fe2(SO4)3 = 399.88 g/mol

mass = mol*MW = 399.88*1.223 = 489.05324 g

b. moles of NH4+ ions in 6.995 g of (NH4)2CO3

MW= 96.09

mol = mass/MW = 6.995 /96.09 = 0.072796336 mol of (NH4)2CO3

since 1 mol of (NH4)2CO3 contains 2 mol of NH4+, then

2*0.072796336 = 0.145592672 mol of NH4+

c. mass in grams of 7.70 x 10^20 molecules of aspirin , C8H10N4O2

change to mol

1 mol = 6.022*10^23

then

n = (7.70*10^20)/(6.022*10^23) = 0.00127

MW = 180.157

mass = mol*MW = 180.157*0.00127 = 0.22879939 g

d. molar mass of diazepam if 0.05570 mol has a mass of 15.85 g

MW = mass/mol = 15.85 /0.05570 = 284.5601 g /mol

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