posted by Kyle
If a sample of Co2(CO)8 is found to contain 6*10^-2 mol of C atoms, how many grams of Co atoms are present?
Molar Mass (g/mol)
Co2(CO)8 - 341.95
Co atom - 58.933
C atom - 12.011
O atom - 15.999
Avaogadro's No.: 6.022*10^23
Do I need to use the 6*10^-2 mol of C atoms to find how many grams are in this sample of Co2(CO)8? Then from there find how many grams of Co atoms?
By the way, for clarification, what does it mean by "how many grams of X atoms?"
The answer is supposed to be: 0.89872825g
But I'd like an explanation on how to do this problem, thank you.
Each molecule contains 2 Co atoms and 8 C atoms. So, divide .06moles of C by 4 to get moles of Co
.06/4 = .015 moles of Co
.015mol * 58.933g/mol = 0.883995g
not quite your answer; check my math.
Why did you divide .06 moles by 4? Is it because there is a 8:4 ratio of C and Co?
Yes (actually a 2:8 ratio). 0.06 mols C x (2 Co atoms/8 mols C atoms) = 0.06 x (2/8) = 0.015 moles Co
I should point out that there is only 1 significant figure in 0.06 mol C atoms in the problem; therefore, an answer of 0.898728..... is inappropriate. The answer of 0.884 should be rounded to 0.9 g Co or 9E-1.