Question

How many molecules of ascorbic acid(vitaminC,
C6H8 O6 )are in a 500 mg
tablet?

Answer 1

Step-by-step explanation:

1) molar mass of the C6H8O6, you need to consult the atomic weight of the C, H and O atoms that are in the periodic table: C is 12; H is 1; O is 16 (12x6)+(1x8)+(16x6)= 176g/mol 176 g = 1 mol 0,5 g = x mol 500mg= 0,5 grams molar mass = mass÷ moles 176 = 0,5÷ x x= 2,84 x 10⁻³ mol 2) To find the number of molecules present in those 2,84 x 10⁻³ mol we need to multiple the moles by the Avogadro's constant No. of molecules = Avogadro's constant x n° of moles No. of molecules = 6.022 x 10²³ x 2,84 x 10⁻³ = 1.71 x 10²¹ molecules of vit C.

Answer 2

1.71 × 10²¹ molecules

Step-by-step explanation:

1 gram is equal to 1000 milligrams. The mass in grams corresponding to 500 mg is:

500 mg × (1 g / 1000 mg) = 0.500 g

The molar mass of ascorbic acid is 176.12 g/mol. The moles corresponding to 0.500 grams of ascorbic acid are:

0.500 g × (1 mol/ 176.12 g) = 0.00284 mol

In 1 mole of ascorbic acid, there are 6.02 × 10²³ molecules of ascorbic acid (Avogadro's number). The molecules in 0.00284 moles are:

0.00284 mol × (6.02 × 10²³ molecules/ 1 mol) = 1.71 × 10²¹ molecule