Question

Part EAscorbic acid, or vitamin C (Ascorbic molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant properties. A healthy adults daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.88 x 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 x 10^4 mol of ascorbic acid.Express the mass in grams to three significant figures.You did not open hints for this part

Answer 1

Step-by-step explanation

Given:

Molar mass of ascorbic acid, M = 176 g/mol

Moles of ascorbic acid in sweet lime = 2.88 x 10⁴ mol

what to find:

The mass of ascorbic acid in 2.88 x 10⁴ mol of ascorbic acid.

Step-by-step solution:

The relationship between mole, n, reacting mass, m, and molar mass, M, is given by

`\text{mole (n) }=\frac{Reac\text{ting mass (}m)}{Molar\text{ mass (}M)}`

So, substitute the given moles and molar mass of ascorbic acid into the formula above to get the mass of ascorbic acid: