Calculate the work (w) and δeo, in kj, at 298 k and 1 atm pressure, for the combustion of one mole of c6h6 (g). first write and balance the equation. the products will be co2 (g) and h2o (g). the value of δho for this reaction is -3169.3 kj/mol.

Answer : The value of w and ΔE is, 1.24 kJ and -3170.5 kJ/mol respectively.

Explanation :

Formula used :

= change in enthalpy  = -3169.3 kJ/mol = -3169300 J/mol

= change in internal energy

= change in moles

R = gas constant = 8.314 J/mol.K

T = temperature = 298 K

The balanced chemical reaction will be:

In this case:

= change in moles

Change in moles = Number of moles of product side - Number of moles of reactant side

According to the reaction:

Change in moles = [3+2] - [1+ (7/2)]= 0.5 mole

Now we have to calculate the work done.

Therefore, the value of w and ΔE is, 1.24 kJ and -3170.5 kJ/mol respectively.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.

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