Vitamin C has the molecular formula of C_6H_8O_. Answer the questions below for

Question

Vitamin C has the molecular formula of C_6H_8O_. Answer the questions below for a 250 mg dose. Show work and answer the questions below (include the units and keep 2 decimal place in the molar mass): A. Calculate the number of moles of Vitamin C in a 250 mg dose: Answer: _______ B. Calculate the number of moles of Oxygen in a 250 mg dose of Vitamin C: Answer: _______ C. Calculate the number of oxygen atoms in a 250 mg dose of Vitamin C Answer: ________ Determine (A) the limiting reactant; and (B) the mass (in g) of H_2O if 50.0 g of methane (CH_4) and 75.0 g of oxygen react according to the following balanced reaction. And finally, determine (C) the percent yield if 40.0 g of H_2O are produced in the reaction. (Possibly useful molar masses: CH_4 = 16.05 g/mol; H_2O = 18.02 g/mol; O_2 = 32.00 g/mol). CH_4(g) + 2 O_2(g) rightarrow CO_2(g)+ 2H_2O(g) A. Circle the limiting reactant: CH_4 O_2 B. Determine the Theoretical yield (mass) of H_2O: Answer: _______ C. Determine the percent yield of H_2O: Answer: _________

Explanation / Answer

A)

moles of Vitamin C in a m = 250 mg dose = 0.250 g

MW of ascorbic acid = 176.12 g/mol

mol = mass/MW = 0.25/176.12 = 0.001419 mol of Vit C

B)

moles of Oxygen in this amount of Vit C

note that the formula has --> C6H8O6

1 mol of Vit C = 6 mol of O

so

0.001419 mol of VitC = 0.001419 *6 = 0.008514 mol of Oxygen

C)

note that

1 mol = 6.022*10^23 atoms

0.008514 moles of Oxygen = (0.008514)(6.022*10^23) = 5.1271*10^21 atoms of Oxygen

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