The formula of ibuprofen is: C13H18O2
The molar mass is:
13x 12.01= 156.13 g/mol of C
18x1.008 = 18.144 g/mol of H
2x16.00 = 32.0 g/mol of O
Total: 206 g/mol of ibuprofen
The molecular formula is C13H18O2, so;
13.5 grams C13H18O2 ( 1mole C13H18O2/206.274 grams )(13 mole C/1 mole C13H18O2)
= 0.8508 moles of carbon
0.8508 mole C ( 12.01 grams/ 1 mole C )
= 10.2 grams of carbon ( reasonable, as carbon is most of this product )
0.200 *(6.02*1023)=1.204*1023 molecules
The number of moles is 0,0157.
33
206
25
The number of moles of carbon in 11,5 g of ibuprofen is 0,725.
Moles of carbon dioxide = grams/amu of carbon dioxide. Moles = 19g/44amu Moles of carbon dioxide = .432
0.1 moles There is one carbon and two oxygens 1 x 0.1 = 0.1
3.5 moles CaCO3 (1 mole carbon/1 mole CaCO3) = 3.5 moles
1.2 Moles
The number of moles of carbon in 11,5 g of ibuprofen is 0,725.
The number of moles of carbon in 11,5 g of ibuprofen is 0,725.
C13H18O2 = ibuprofen 7.4 X 1025 carbon atoms (1 mole C atoms/6.022 X 1023)(1 mole ibuprofen/13 mole carbon) = 9.5 moles ibuprofen ------------------------------
Molar mass of ibuprofen is = 206g/mole 0.525 moles ibuprofen x (206g ibuprofen/1mole ibuprofen) = 108g ibuprofen
Moles of carbon dioxide = grams/amu of carbon dioxide. Moles = 19g/44amu Moles of carbon dioxide = .432
0.1 moles There is one carbon and two oxygens 1 x 0.1 = 0.1
211g of carbon dioxide are equal to 4,794 moles.
19
About one half mole. 6 grams carbon (1 mole C/12.01 grams) = 0.4996 moles of carbon --------------------------------- that is, 0.5 moles carbon ---------------------------------
3.5 moles CaCO3 (1 mole carbon/1 mole CaCO3) = 3.5 moles
10 g of carbon is equivalent to 0,8326 moles.
0,515 g of carbon is equal to 0,043 moles.