Question

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 2.82×10−4 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 2.82×10−4 mol of ascorbic acid.

Answer 1

The mass of ascorbic acid in a sweet lime, which contains 2.82×10⁻⁴ mol of ascorbic acid, is approximately 49.6 mg. This is within the daily requirement of 70-90 mg for a healthy adult.

Step-by-step explanation:

To calculate the mass of ascorbic acid in 2.82×10⁻⁴ mol of ascorbic acid, we use the formula:

Mass = moles × molar mass

Given that the molar mass of ascorbic acid (C6H8O6) is 176 g/mol, we can calculate the mass as follows:

Mass = (2.82×10⁻⁴ mol) × (176 g/mol) = 4.96×10⁻² g

To convert this to milligrams (mg), we remember that 1 gram is equivalent to 1000 mg:

Mass in mg = 4.96×10⁻² g × 1000 mg/g = 49.6 mg

Therefore, a sweet lime contains approximately 49.6 mg of ascorbic acid, which is within the healthy adult daily requirement of 70–90 mg.

Answer 2

49.7 mg of Ascorbic acid do not meet the daily requirement.

Step-by-step explanation:

The conversions are

Moles to mass, by multiplying with molar mass.

Molar mass is the mass of 1 mole of the substance.

Its unit is gram per mole g/mol

Ascorbic acid (
`C_6H_8O_6`) contains 6, C atoms 8, H atoms and 6, O atoms .

We find the molar mass of the compound by just adding the atomic mass of the atoms present in it

Molar mass of Ascorbic acid

`=(6* 12.0107)+(8* 1.00784)+(6* 15.999)`

=176.124 g/mol(Given)

Mass of Ascorbic acid = Moles × Molar mass

`=2.82 * 10^(-4) mol * 176.124 g/mol`

=0.0497 g

We know

1 g = 1000 mg

So

`0.0497g * 1000mg/1g=49.7mg` VITAMIN C

The required quantity for an Adult is 70 to 90mg.

So 49.7 mg of Ascorbic acid do not meet the daily requirement.(Answer)