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Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant properties. A healthy adult’s daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.88×10−4 mol of ascorbic acid. To determine whether the ascorbic acid in a sweet lime meets the daily requirement, calculate the mass of ascorbic acid in 2.88×10−4 mol of ascorbic acid.

Respuesta :

Answer : 50.69 mg of ascorbic acid does not meet the daily requirement.

Solution : Given,

Molar mass of Ascorbic acid = 176 g/mole

Moles of Ascorbic acid = [tex]2.88\times 10^{-4}moles[/tex]

Formula used :

[tex]Moles=\frac{Mass}{\text{ Molar mass}}[/tex]

or, [tex]\text{ Mass of ascorbic acid}=\text{ Moles of ascorbic acid}\times \text{ Molar mass of ascorbic acid}[/tex]

Now put all the given values in this formula, we get the mass of ascorbic acid.

[tex]\text{ Mass of ascorbic acid}=(2.88\times 10^{-4}moles)\times (176g/mole)=0.050688g=50.69mg[/tex]

Conversion : [tex](1g=1000mg)[/tex]

As per question, a healthy adult’s daily requirement of vitamin C is 70-90 mg. But calculate mass of vitamin C is 50.69 mg. So, 50.69 mg of ascorbic acid does not meet the daily requirement.

Bribri47825

Answer:

5.07×10^-2

Explanation:

in case they want it to be written out instead of the plain answer

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