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

b..

is the correct one

explanation:

covalent bonds form as valence electrons are shared between two atoms. lewis structures and structural formulas are common ways of showing the covalent bonding in organic molecules. formal charge describes the changes in the number of valence electrons as an atom becomes bonded into a molecule.

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