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.

uranium-238 i believe is your answer

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