Molecular formula of ascorbic acid is [tex] C_{6}H_{8}O_{6} [/tex]
Molar mass of ascorbic acid = [tex] (6 * 12 g/mol) + (8 * 1 g/mol) + (6 * 16 g/mol) = 176 g/mol [/tex]
Converting 500.0 mg of ascorbic acid to moles: We use molar mass of ascorbic acid to convert mass to moles.
[tex] 500.0 mg * \frac{1 g}{1000 g} *\frac{1 mol}{176 g} = 0.00284 mol [/tex]
Converting 500.0 mg of ascorbic acid to molecules: The conversion factor used is 1 mole = [tex] 6.022*10^{23} molecules [/tex]
[tex] 500.0 mg * \frac{1 g}{1000 mg}*\frac{1 mol}{176 g} * \frac{6.022*10^{23}molecules}{1 mol} = 1.71 * 10^{21} molecules [/tex]
Answer:
Molar mass of ascorbic acid is 176 g.
The tablet contains 0.002841 moles and [tex]1.711\times 10^{21}[/tex] molecules of vitamin C.
Explanation:
Molar mass of vitamin C=[tex](6\times atomic mass of C)+(8\times atomic mass of H)+(6\times atomic mass of O)[/tex] = [tex](6\times 12 g)+(8\times 1 g)+(6\times 16 g)[/tex] = 176 g
We know, number of moles = [tex]\frac{mass}{molar mass}[/tex]
So moles of vitamin C in 500.0 mg tablet = [tex]\frac{0.5000 g}{176 g}[/tex]
= 0.002841 moles
We know 1 mol of a compound contains [tex]6.023\times 10^{23}[/tex] molecules of that compound.
So number of molecules of vitamin C in 500.0 mg tablet = [tex]0.002841\times 6.023\times 10^{23}[/tex] molecules = [tex]1.711\times 10^{21}[/tex] molecules
