Calculate the amount of energy in the form of heat that is produced when a volume of 3.43 l of so2(g) is converted to 3.43 l of so3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °c . assume ideal gas behavior.

Explanation:

The reaction equation will be as follows.

And, the standard enthalpies of formation for and are as follows.

  = -296.8 kJ/mol

  = -395.7 kJ/mol

Now, according to the ideal gas equation PV = nRT.

    Number of moles of 3.43 L of =

             =               (as 1 bar = 1 atm (approximately))

             = 0.140

Now, no. of moles of 3.43 L of are also 0.140.

Hence, calculate the enthalpies of formation for 0.140 moles of and as follows.

        and

    and respectively.

or,                  

                          =

                         = 13.84 kJ

Therefore, we can conclude that the amount of energy in the form of heat that is produced is 13.84 kJ.

it takes on an electronical energy

a is the correct answer