Question

What is the mass, in grams, of Vitamin C (C6H8O6) that contains 1.076 grams of carbon?

Answer 1

`2.63\ \text{g}`

Step-by-step explanation:

Mass of carbon = 1.076 grams

Moles of carbon =
`(1.076)/(12)=0.08967\ \text{mol}`

1 Mol of vitamin C = 6 moles of carbon

`0.08967\ \text{mol}` = 6 moles of carbon

Moles of vitamin C =
`(1)/(6)* 0.08967=0.014945\ \text{mol}`

Molar mass of vitamin C =
`12*6+1.00794* 8+16* 6=176.06352\ \text{g/mol}`

Mass of vitamin C

`\text{Moles of vitamin C}* \text{Molar mass of vitamin C}\\ =0.014945* 176.06352 \\ =2.63\ \text{g}`

The mass of vitamin C is
`2.63\ \text{g}`