Question

Problem 1 (a) (1 point) Balance the ideal combustion of ethanol, C2H5OH, with air (b) (1 point) How many pounds of CO2 are produced for each ton of ethanol that is burned? Given molecular mass of C = 12.0 g/mol, H = 1.0 g/mol, and O = 16.0 g/mol. (c) (1 point) The heat of combustion of ethanol is 13,180 Btu/lb. Calculate the heat released upon burning one ton of ethanol. (d) (1 point) How many pounds of CO2 are produced per million Btu of heat released by burning ethanol? (e) (1 point) It is known that gasoline produces 150 pounds of CO2 per million Btu of heat released. Suppose Congress were to pass a law requiring automobiles to burn ethanol instead of gasoline. Would such a law reduce CO2 emissions from automobiles by at least 5%? Explain. Problem 2 a. (3 points) Construct the balanced equation for the combustion of dodecane (C12H26) with 20% excess air but where only 90% of the carbon is combusted to CO2. b. (2 points) How many tons of carbon monoxide (CO) are produced for each ton of dodecane that is burned?

Answer 1

PROBLEM- 1

a) Ethanol, C2H5OH burns with oxygen in air to give carbon dioxide and water. what is the amount (in moles) of water produced from 0.51 mol C2H5OH. the equation is -

C2H5OH + 3O2 -----> 2CO2 + 3H2O.

I lon - 9071859 Spound = 453.59 g 5 1 pound – 0.0005. Con CHO H + 30 - 200 + 3H₂007 Imol ethanol produces 2 mol CO2 46.07 g . " (44x2g) Co₂ (9091859) » ».44x2 x 9071897 9.60 46.07 2 1732847.49cc 173 2844.41453.51 ound. 3620 pound: & -(e): 1 pound - 13, 180 Btu heal of combustion So, 0.0005 ton = 13180 Blu ) + 1 ton = 13186 0.0005 26360000 Blu