How many molecules of ascorbic acid (vitamin c, c6h8o6) are in a 500 mg tablet?

1.71 x 10²¹ molecules of ascorbic acid.

Further explanation

The Problem:

What is the number of molecules of ascorbic acid (vitamin C or C₆H₈O₆) found in a 500 mg tablet?

The Process:

Step-1

Calculate the molar mass of ascorbic acid or C₆H₈O₆.

Rounding the relative atomic mass gives us:

• C = 12 g/mol
• H = 1 g/mol
• O = 16 g/mol

Ascorbic acid consists of six carbon atoms, eight hydrogen atoms, and six oxygen atoms, leading to a molar mass of

Step-2

Next, we will determine the number of moles in 500 mg of ascorbic acid by converting it into grams, which is 0.5 g.

This results in 2.84 x 10⁻³ moles.

Step-3

It’s important to note that one mole is equivalent to 6.02 x 10²³ molecules, known as Avogadro's number.

Now let's convert 2.84 x 10⁻³ moles to the total number of molecules (N).

Hence, the total number of molecules in a 500 mg tablet of C₆H₈O₆ is .

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Quick Steps

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1) To find the molar mass of C6H8O6, you must refer to the atomic weights of C, H, and O from the periodic table: C is 12; H is 1; O is 16 <span> (12x6)+(1x8)+(16x6)= 176g/mol


</span> <span> 176 g = 1 mol
0.5 g = x mol = 500 mg = 0.5 grams

Molar mass = mass ÷ moles
176 = 0.5 ÷ x
x = 2.84 x 10⁻³ mol
2) To calculate the total number of molecules in those </span> 2.84 x 10⁻³ mol, multiply the moles by <span> Avogadro's constant.
Number of molecules = Avogadro's constant x number of moles
Number of molecules = 6.022 x 10²³ x 2.84 x 10⁻³ </span> = 1.71 x 10²¹ molecules of vitamin C. <span>
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