Find δh for the combustion of ethanol (c2h6o) to carbon dioxide and liquid water from the following data. the heat capacity of the bomb calorimeter is 34.65 kj/k and the combustion of 1.752 g of ethanol raises the temperature of the calorimeter from 294.42 k to 295.92 k .

Answer : The enthalpy of combustion of ethanol is, -1366.8 KJ/mole

Explanation :

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

First we have to calculate the heat released by calorimeter.

where,

= heat released by calorimeter = ?

c = heat capacity of bomb calorimeter =

m = mass of ethanol = 1.752 g

= initial temperature of calorimeter = 294.42 K

= final temperature of calorimeter = 295.92 K

Now put all the given values in the above formula, we get

Now we have to calculate the moles of ethanol.

Now we have to calculate the enthalpy of combustion of ethanol.

where,

= enthalpy of combustion = ?

q = heat released = -51.98 KJ

n = number of moles used in combustion = 0.03803 mole

The negative sign indicate the heat released during the reaction.

Therefore, the enthalpy of combustion of ethanol is, -1366.8 KJ/mole

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

if you need further assistance, let me know: )

~ trueboss72