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
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.
To answer these questions, you need to understand the concept of bond energy and how to calculate the total energy change in a chemical reaction.
1. For each type of bond, you need to determine the number of bonds broken and formed in the reaction. The number of bonds is indicated by the coefficients in front of the chemical formulas of the reactants and products. For example, in the reaction 2(H—C ≡ C—H), there are two C≡C bonds broken and two C—H bonds formed.
2. The bond energies for each type of bond can be found in a reference source. These energies represent the amount of energy required to break one mole of a particular bond in a gaseous molecule. The given values for the bond energies in kJ/mol are:
- C≡C bond energy: 839 kJ/mol
- O=O bond energy: 495 kJ/mol
- C—H bond energy: 413 kJ/mol
- C—O bond energy: 358 kJ/mol
- H—O bond energy: 467 kJ/mol
3. To calculate the energy change in the reaction, you need to use the difference between the total energy of the reactants and the total energy of the products. The energy change is given by:
Energy change = (sum of bond energies in reactants) - (sum of bond energies in products)
Now let's answer the questions using the above information and steps:
- C≡C # of bonds: 2
- O=O # of bonds: 5
- C—H # of bonds: 2
- C—O # of bonds: 4
- H—O # of bonds: 2
- Energy change on the reactant side: Calculate the sum of the bond energies for the reactants. For example:
Energy = 2(C≡C bond energy) + 5(O=O bond energy)
- Energy change on the product side: Calculate the sum of the bond energies for the products. For example:
Energy = 4(C—O bond energy) + 2(H—O bond energy)
- Whether the reaction is endothermic or exothermic depends on the sign of the energy change. If the value is negative, the reaction is exothermic (releases energy). If the value is positive, the reaction is endothermic (absorbs energy).
- To calculate the energy produced or absorbed when a certain number of moles of acetylene (C2H2) react, you need to know the stoichiometry of the reaction. The coefficients in front of the reactants and products give you the mole ratio. Use this ratio to calculate the amounts of reactants and products, and then multiply this value by the energy change per mole to determine the energy change for the given number of moles.
Please provide the coefficients (numbers) in the balanced equation for the given number of moles of acetylene reacting to proceed further.
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.
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 !
Ah, chemistry! Let's break it down step by step, and I'll help you fill in the blanks with some humorous explanations.
First, let's determine the number of bonds for each compound:
C ≡ C (acetylene) means there is a triple bond between two carbon atoms. So, the number of bonds is 3.
O = O (oxygen) has a double bond, so the number of bonds is 2.
C—H (carbon-hydrogen) has a single bond, so the number of bonds is 1.
C—O (carbon-oxygen) also has a single bond, so the number of bonds is 1.
H—O (hydrogen-oxygen) also has a single bond, so the number of bonds is 1.
Now let's fill in the blanks with some humorous explanations for the energy:
(product/reactant) side Energy:
For C ≡ C: "It takes more energy to break a triple bond, like breaking up your favorite trio of singing chipmunks. So, let's say it's like trying to convince Alvin, Simon, and Theodore to go their separate ways. Put 839 kJ/mol on the reactant side, because it's not easy separating them."
For O = O: "Breaking up a double bond, you know, like trying to split a delicious sandwich into two average sandwiches. It requires less effort. So, put 495 kJ/mol on the reactant side."
For C—H: "Just a regular single bond, kind of like matching socks – easy to separate. Add 413 kJ/mol to the reactant side."
For C--O: "Another single bond, like the bond between you and your pet clownfish. Place 358 kJ/mol on both the product and reactant side."
For H--O: "Yet again, a single bond, like a blissful relationship between you and your rubber ducky. Add 467 kJ/mol on both the product and reactant side."
Now, let's add up the energies:
Add the energies on the reactant side: 839 + 5(495) + 2(413) = _____
Add the energies on the product side: 4(358) + 2(467) = _____
This reaction is (endothermic/exothermic):
To determine if it's endo or exo, think about how you feel after eating a spicy taco. If it's exothermic, the reaction releases energy like a spicy taco releasing heat. So, is it exothermic or endothermic?
The reaction (produces/absorbs) _____ kJ when ____ moles of acetylene (C2H2) reacts:
Multiply the energy value that you found on the product side by the number of moles of acetylene reacting. Fill in the blanks with the correct terms and numbers!
Hope this helps add a dash of humor to your chemistry questions!