Q 8.67

Moderators: Chem_Mod, Chem_Admin

Rucha Kulkarni 2A
Posts: 43
Joined: Fri Sep 29, 2017 7:05 am

Q 8.67

Postby Rucha Kulkarni 2A » Sun Jan 14, 2018 8:08 pm

Does anyone know how to solve exercise 8.67 from the homework?

Riya Pathare 2E
Posts: 74
Joined: Sat Jul 22, 2017 3:01 am
Been upvoted: 1 time

Re: Q 8.67

Postby Riya Pathare 2E » Mon Jan 15, 2018 12:19 pm

You need to first make the balanced equation of how the products form from their elemental forms because we are trying to find standard enthalpy of formation which means the products must be elemental forms. Then use the bond enthalpies and subtract the energy released when creating the new product bonds from the energy needed to break each of the bonds in the reactants. For example for part A the equation is H2 + 1/2 O2 -> H20. In this case we need to break one H2 bond and 1/2 of an O2 bond and for two O--H bonds. Thus we do (436 kJ + 1/2(496kJ)) - (2(463kJ)) based on the bond enthalpies in the tables.

Anna Goldberg 2I
Posts: 59
Joined: Fri Sep 29, 2017 7:04 am
Been upvoted: 1 time

Re: Q 8.67

Postby Anna Goldberg 2I » Tue Jan 16, 2018 12:37 pm

After you do the above calculations with the bond enthalpies, you should have delta H = -242 kJ/mol.
You then need to take into account that water is in it's gaseous phase here, and the question asks for you to find the enthalpy of formation at a liquid state.
With this in mind, subtract the enthalpy of vaporization, which is 44 kJ/mol, from -242 kJ/mol, to get the answer of -286 kJ/mol.

Return to “Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)”

Who is online

Users browsing this forum: No registered users and 3 guests