2. Vitamin C has a formula of C6H8O6.
a. The recommended daily dose of vitamin C is 60 mg. How many moles are you consuming if you ingest 60 mg of the vitamin?
b.A typical tablet contains 1.00g of vitaminC. How many moles of vitaminC does this represent?
c. When you consume 1.00g of vitaminC, how many oxygen atoms are you eating?
Please, any help with this question will be greatly appreciated; if possible show the steps you did to get the answer.
2007-01-21 14:56:14 · 4 answers · asked by j a 1 in Science & Mathematics ➔ Chemistry
Question 1. Get your units of body weights in kg.
145 lb is about 70 kg. Then Dose= dose/kg x kgs
2a. Find mole weight of vit A.
12x6 (for C) + 8x1 (for H) + 16x6 (for O). I get 176 g/mole. So 60 mg is about 0.00029 moles.
b. Since 176 g=1 mole, 1 g= 1/176 mole
c. 1 mole of Vit A provides 6 g-atoms of O.
so 6 g-atoms would be 6x6.02x10(exp23) atoms
Divide by 176 to get your answer.
2007-01-21 15:13:08 · answer #1 · answered by cattbarf 7 · 0⤊ 0⤋
first one is
7.5 g/ 2.2 lbs X 145 lbs = 494 g for fatal dose.
I think the others need to take amu X avagadros number to see how many moles. But my chemistry classes were decades ago.
2007-01-21 23:07:02 · answer #2 · answered by Anonymous · 1⤊ 0⤋
1 kg = 2.2 pounds
145 / 2.2 = 65.91 kg
65.91 kg x 7.5 g/kg = 494.325 g
2007-01-21 23:05:02 · answer #3 · answered by Anonymous · 1⤊ 0⤋
one kilo is 2.2 pounds, you do the math.
2007-01-21 22:59:32 · answer #4 · answered by wwhrd 7 · 0⤊ 1⤋