In each mole of ethanol there are two moles of carbon atoms. One mole of carbon atoms is required to form one mole of carbon dioxide, so two moles will form two moles. Thus each mole of ethanol completely combusted will form two moles of carbon dioxide.
Balanced equation.
2C2H2 + 5O2 -> 4CO2 + 2H2O
O2 is assumed to be in excess
1 mole C2H2 (4 mole CO2/2 mole C2H2)
= 2 moles CO2 produced
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The answer is 16,5 moles carbon dioxide.
1.5 - your welcome
The total number of moles of NO produced when 1,0 mole of O2 is completely consumed is 2.
11,2 moles carbon dioxide are obtained.
6 moles COULD be produced
1,4 moles of CO are produced.
It forms H2O when burned.There are 3.744 moles of H2O after burned.
6,49 moles of water are obtained.
If burnt with excess O2 then 19.65 (=3*6.55) mole H2O
1.5 - your welcome
30 moles
For this you need the atomic (molecular) mass of C2H5OH. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel. C2H5OH= 46.1 grams1.271 grams C2H5OH / (46.1 grams) = .0276 moles C2H5OH
2
The total number of moles of NO produced when 1,0 mole of O2 is completely consumed is 2.
11,2 moles carbon dioxide are obtained.
0.4 moles MgO
.913 moles
Balanced equation first, 2C6H14 + 19O2 >> 12CO2 + 14H2O 84.4 moles hexane (12 moles CO2/2 moles C6H14) = 506.4 moles of CO2