Antacid tablets, such as tums, are mainly calcium carbonate. calculate the mass of a tums tablet which contains 1000 mg of calcium.

The formula for calcium carbonate is

CaCO3

So each mole of calcium carbonate contains one mole of calcium

Molar mass of calcium carbonate = 100g/mole

Atomic mass of calcium = 40g/ mole

Hence if 40g of calcium is present it means we have 100g of calcium carbonate

if 1 g of calcium is present it means we have 100/ 40 g of calcium carbonate

So if 1000 mg of calcium is present = 100 X 1000 / 40 mg of CaCO3 is present

                                                          = 2500 mg of CaCO3 in tum tablets

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.