Telling me you don't have any idea doesn't help much. It would help if I knew exactly what it is you don't undersand but let me see if I can get you started. I won't do the entire problem.
First, I assume the equation is this and note that I've change the CO2 part. If that isn't correct just ignore everything that follows.
2(H—C ≡ C—H) + 5(O = O) → 4 (O=C=O) + 2 (H—O—H)
The first question is how many C ≡ C bonds. You have 1 per mole and you have 2 moles (coefficient of 2 tell you that). So the number of C ≡ C is 2.
It takes 839 kJ/mol to break the C ≡ C; therefore, it will take 2 moles*839 kJ/mo = 1678 kJ energy to break those moles of C ≡ C and that's on the reactant side so you're to underline or cirlce reactant. Next part. 495 kJ/mol for O=O bond. How many bonds? That is 5. They are on the reactant side so circle that. Thje 5 moles x 495 kJ/mo = 2475 kJ for the 5 moles O2.
Next. 413 kJ/mol for C-H bonds. You have two C-H bonds/mole x 2 mols = 4 moles C-H @ 413 each = 1652 kJ for th four C-H bonds and circle reactant side. You should have the idea by now. You do the same process for the product side where you write in the number of bonds, the total energy for forming those bonds and circle product side for those.
Then you add the energy to break the bonds on the reactant side (if I've done the math right you shoud get 5805 kJ. Check that. Add the values on the product side. That's the amount of energy you get by forming those bonds.
The final steps which the problem could have made easier by showing how to get that. Here is what you do. Energy to break bonds on reactant side minus energy to form bonds on the product side = bond energy for the reaction. There is no place for you to put that number but it is essential that you have that number. All of that work at the beginning is to arrive at the bond energy for the reaction. For the rest of the table here are the rules.
If the bond energy for the reaction is + it is endothermic. If the bond energy is - the reaction is exothermic. If the reaction is exothermic it produces. If the reaction is endothermic it absorbs. Hope this helps. If you do a follow up please explain as much as you can about where the problem is in detail. I can do a better job if I know where I'm going. By the way, you need not share this with your instructor but I wish this was not taught in school. In my opinion, it is useless and there are easier and more accurate ways to get the same end information. Delta Ho formation gives the same information and it is far more accurate. These bond energy data are averages and ONLY useful for gases.
2(H—C ≡ C—H) + 5(O = O) → 4 (O—C—O) + 2 (H—O—H)
839 kJ/mol C ≡ C # of bonds ______
(product / reactant) side Energy:_____
495 kJ/mo O = O # of bonds ______ (product / reactant) side Energy:_____
413 kJ/mo C—H # of bonds ______ (product / reactant) side Energy:_____
358 kj/mol C--O # of bonds _____(product/reactant) side Energy:_____
467 kj/mol H--O # of bonds _____(product/reactant) side Energy:_____
Add the energies on the reactant side _____ kj/mol
Add the energies on the product side____ kj/mol
This reaction is (endothermic/exothermic)
The reaction (produces/absorbs) _____ Kj when ____ moles of acetylene (c2h2) reacts.
What exactly am I supposed to do? How do I answer this? I have no idea how to fill this in or what its asking me to do, please help
3 answers
Thank you so much Dr Bob, from the assignment thats all that there was to the question so thats why I was very confused . There wasent too much information from the question itself but I understand it a bit better now so I very much appreciate it !
Of the bonds listed below the weakest bond is C-O and the strongest is C=C.
A strong bond is a stable bond
2(H—C ≡ C—H) + 5(O = O) → 4 (O—C—O) + 2 (H—O—H)
839 kJ/mol C ≡ C # of bonds __2 __ reactant side Energy:1678 kg/mol
495 kJ/mo O = O # of bonds __5_ reactant side Energy:_2475 kg/mol
413 kJ/mo C—H # of bonds __2__ reactant side Energy:_1652 kg/mol
358 kJ/mo C—O # of bonds __8__ product side Energy:__2864 kg/mol
467 kJ/mo H—O # of bonds __4__ product side Energy: 1868 kg/mol
Add the energies on the reactant side _5805 kJ/mol
Add the energies on the product side _4732 kJ/mol
This reaction is endothermic
The reaction produces 1073 kJ when 2 moles of acetylene (C2H2) reacts.
A strong bond is a stable bond
2(H—C ≡ C—H) + 5(O = O) → 4 (O—C—O) + 2 (H—O—H)
839 kJ/mol C ≡ C # of bonds __2 __ reactant side Energy:1678 kg/mol
495 kJ/mo O = O # of bonds __5_ reactant side Energy:_2475 kg/mol
413 kJ/mo C—H # of bonds __2__ reactant side Energy:_1652 kg/mol
358 kJ/mo C—O # of bonds __8__ product side Energy:__2864 kg/mol
467 kJ/mo H—O # of bonds __4__ product side Energy: 1868 kg/mol
Add the energies on the reactant side _5805 kJ/mol
Add the energies on the product side _4732 kJ/mol
This reaction is endothermic
The reaction produces 1073 kJ when 2 moles of acetylene (C2H2) reacts.