If hydrogen were used as a fuel, it could be burned according to this reaction:
Use average bond energies to calculate for this reaction and also for the combustion of methane (CH4). Which fuel yields more energy per mole? Per gram?
Solution 105E Step 1 of 4 For the reaction Thus we can see that at the end of this reaction one HH bond and 1/2 O=O bond are broken and 2 bonds OH are formed.We have to remember that when a reaction happens, we have to spend energy to break bonds (positive H ), while broken bonds release energy (negative H) Since For H-H H = 436 kJ/mol For O=O H = 498 kJ/mol Thus H broken bonds= (H H-H)+ 1/2 (H O=O)= 685 kJ/mol For O-H H = -464 kJ/mol Thus H formed bonds= 2(H O-H)= -928 kJ/mol Since H RXN (H broken bonds) + (H formed bonds) H RXN (685 kJ/mol) + (- 928 kJ/mol)= -243 kJ/mol This means that 1 mol of H re2ases 243 kJ. Step 2 of 4 We can even obtain the value per gram of H divid2g the value of H RXNfor the Molar mass (the mass of 1 mol) of H : 2 [-243 kJ/mol/ (2.016 g/mol)] = -121.5 kJ/g
Textbook: Chemistry: A Molecular Approach
Author: Nivaldo J. Tro
This full solution covers the following key subjects: Fuel, reaction, according, Bond, burned. This expansive textbook survival guide covers 82 chapters, and 9454 solutions. The full step-by-step solution to problem: 105E from chapter: 9 was answered by , our top Chemistry solution expert on 02/22/17, 04:35PM. Since the solution to 105E from 9 chapter was answered, more than 597 students have viewed the full step-by-step answer. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3. The answer to “If hydrogen were used as a fuel, it could be burned according to this reaction: Use average bond energies to calculate for this reaction and also for the combustion of methane (CH4). Which fuel yields more energy per mole? Per gram?” is broken down into a number of easy to follow steps, and 41 words.