Consider the reaction 2h2o(g) → 2h2(g) + o2(g)δh = 483.6 kj/mol. if 2.0 moles of h2o(g) are converted to h2(g) and o2(g) against a pressure of 1.0 atm at 165°c, what is δu for this reaction?

Answer : The value of of the reaction is, 479.958 KJ/mole

Explanation :

The relation between the internal energy and enthalpy of reaction is:

where,

= internal energy of the reaction = ?

= enthalpy of the reaction = 483.6 KJ/mole = 483600 J/mole

From the balanced reaction we conclude that,

= change in the moles of the reaction = Moles of product - Moles of reactant = 3 - 2 = 1 mole

R = gas constant = 8.314 J/mole.K

T = temperature =

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

Therefore, the value of of the reaction is, 479.958 KJ/mole

where is the following

explanation: