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3 days ago

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

Chemistry

2 answers:

Tems11 [2.6K]3 days ago

8 0

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

$\boxed{(12 \times 6) + (1 \times 8) + (16 \times 6) = 176 \ g/moles}$

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.

$\boxed{ \ moles = \frac{mass}{molar \ mass} \ } \rightarrow \boxed{ \ moles = \frac{0.5 \ g}{176 \ g/mol} \ }$

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).

$\boxed{ \ moles = \frac{N}{6.02 \times 10^{23}} \ } \rightarrow \boxed{ \ N = moles \times 6.02 \times 10^{23} \ }$

$\boxed{ \ N = 2.84 \times 10^{-3} \ moles \times 6.02 \times 10^{23} \ \frac{molecules}{mol} \ }$

Hence, the total number of molecules in a 500 mg tablet of C₆H₈O₆ is $\boxed{ \ 1.71 \times 10^{21} \ molecules \ }$ .

- - - - - - -

Quick Steps

$\boxed{ \ \frac{6.02 \times 10^{23} \ molecules}{1 \ mol} \times \frac{1 \ mole}{176 \ gram} \times 0.5 \ grams \ } = \boxed{ \ 1.71 \times 10^{21} \ molecules \ }$

Learn more

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eduard [2.6K]3 days ago

6 0

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 (12x6)+(1x8)+(16x6)= 176g/mol

 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 2.84 x 10⁻³ mol, multiply the moles by 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 = 1.71 x 10²¹ molecules of vitamin C.

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