Ethanol is a possible fuel. use average bond energies to calculate δhrxn for the combustion of ethanol. ch3ch2oh(g) + 3 o2(g) → 2 co2(g) + 3 h2o(g) express your answer as an integer.

Explanation:

The reaction is as follows.

       

Standard values of bond energies are as follows.

C-C = 347 kJ/mol

C-H = 414 kJ/mol

C-O = 360 kJ/mol

O-H = 464 kJ/mol

O=O = 498 kJ/mol

C=O = 799 kJ/mol

Hence, calculate the change in enthalpy of the reaction as follows.

 

= [5(C-H) + 1(C-C) + 1(C-O) + 1(O-H) + 3(O=O)] - [4(C=O) + 6(O-H)]

 =

       = (4735 - 5980) kJ

       = -1245 kJ

Thus, we can conclude that the enthalpy of given reaction is -1245 kJ.

Ch4 is nonpolar and insoluble in water. since all of the hydrogen atoms are evenly spread around the carbon atom even through the c h bond is polar all the poles cancel each other out.

So what you would do is go through and add 3 teaspoons(tsp) 6 times because of the 6 tablespoons(tbsp). which will give you an answer of 18. another way is to multiply 3x6=18.