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Help with Mass- Volume Gas Law Mole Problem?
How many liters of carbon dioxide are produced when 10.0 ml of ethyl alcohol (C2H5OH) are burned completely in oxygen? the density of ethyl alcohol is 0.789 g/ml
please show the work as best you can... thank you in advance!
4 Answers
- drbillmacmoLv 61 decade agoFavorite Answer
0.789 g/mL x 10.0 mL = 7.89g EtOH
7.89g EtOH x (1 mole EtOH / 40.021g EtOH) = 0.171 moles EtOH
C2H5OH + 3O2 ==> 2CO2 + 3H2O
0.171 moles EtOH x (2 moles CO2 / 1 mole EtOH) = 0.343 moles CO2
Assuming STP
0.343 moles CO2 x (22.4L CO2 / 1 mole CO2) = 7.68L CO2
- ?Lv 45 years ago
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T temperature to be measured on kelvin scale.. i.e. 19+273 ok and no of moles.. weight divided via molecular weight fee of R 2 b chosen accordin to the instruments used for pressur en volume.. if u use atm-l then the fee of R is 0.0821 if u use pascal-m^3 fee is 8.314 and for calculation of heat or potential in energy, fee of R shud be approximated to 2
- 1 decade ago
mass of C2H5OH = 10 mL * 0.789 g/mL = 7.89 g
Mr C2H5OH = 46
mol C2H5OH = 7.89 g : 46 g/mol = 0.17 mol
The reaction :
C2H5OH + 7/2O2 ---> 2CO2 + 3H2O
0.17 mol
mol CO2 = 2 * 0.17 mol
= 0.34 mol
volume CO2 (STP) = 0.34 mol * 22.4 L/mol
= 7.616 L
