the complete combustion of ethanol produces carbon dioxide and water according to the following chemical equat

Question

the complete combustion of ethanol produces carbon dioxide and water according to the following chemical equation: C2H5OH(l) + 3O2(g) + 3H2O(l)

how many grams of carbon dioxide are produced when 1.2 moles of water are produced?

Answer 1

The balanced equation is:

C2H5OH (l) + 3 O2 (g) --> 2 CO2 (g) + 3 H2O (g)

The ratio of CO2 produced to Water produced is: 2/3

If 1.2 moles of water are produced, then

1.2 * 2/3 = 0.80 moles of CO2 are produced.

0.80 moles * 44.01 g/mole = 35.21 grams of CO2

Answer 2

if 1.2 moles of H2O are produced then you take
1.2mol H2O x 1mole C2H5OH/3 mol H2O because C2H5OH to H2O is a 1to 3 ratio
so you have .4 mole of C2H5OH

then you take the number of moles times the molar mass of C2H5OH over one mole

.4molx( 46.07g/1mol)=18.43g of C2H5OH

Answer 3

the most promising answer lies in image voltaic potential. image voltaic cells are expanding in performance each and each year. even as they do attain a particular performance, you'll start up to make certain genuine replace contained in the global. the reason of it truly is because image voltaic potential will produce ability for more good value than classic fossil fuels.And carbon emissions will be critically decreased even as this happens.