Concept explainers
Interpretation:
Using the given bond energy values check whether the hydrogen really a good fuel or not and also check the calculated value of hydrogen matches to the given equation or not.
Concept Introduction:
Energy of Combustion: The energy released in the form of heat when given substance undergoes combustion reaction.
A Fuel is a substance that releases energy when it gets burnt in presence of Oxygen. The phenomenon a substance getting burnt in presence of Oxygen is termed as combustion and it is exothermic process. The larger the amount of heat released per gram of a substance, greater the potential it has to be a fuel.
Exothermic reaction: Exothermic reactions are those in which evolution of heat takes place during any
Endothermic reaction: Endothermic reactions are those in which heat is absorbed during any chemical reaction. In such type of reactions, external energy is needed
Want to see the full answer?
Check out a sample textbook solutionChapter 7 Solutions
Chemistry In Context
- hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?arrow_forwardGiven the following data calculate H for the reaction On the basis of the enthalpy change, is this a useful reaction for the synthesis of ammonia?arrow_forwardUse average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. C2H4(g) + Br2(g) CH,BRCH,Br(g) To analyze the reaction, first draw Lewis structures for all reactant and product molecules. • Include all valence lone pairs in your answer. • Draw the reaction using separate sketchers for each species. One molecule per sketcher, please. Separate multiple reactants and/or products using the + sign from the drop-down arrow. Separate reactants from products using the If you have to draw H,, draw H-H. • Be sure that your structural equation is balanced. symbol from the drop-down menu.arrow_forward
- The average bond enthalpy for C−H is 413 kJ/mol. 413 kJ of energy is required to break a mole of CH into atoms: CH(g)→C(g)+H(g), ΔH=413 kJ Using this information, and your answer from Part A, calculate the enthalpy change of the reaction from Part B. That is, calculate the energy required to break only the carbon-carbon bonds in benzene. PART A ANSWER ΔH∘rxn = 5535.1 kJ.. PART B ANSWER C6H6(g)→6CH(g)arrow_forwardCarbon dioxide in the atmosphere is considered a major contributor to global warming. Its Lewis structure is simple, as shown below. The nonbonding electrons in this Lewis structure are missing. How many pairs of nonbonding electrons are missing in the provided Lewis structure for carbon dioxide? (note, you are asked for pairs of nonbonding electrons, not the total individual nonbonding electrons). O=C=O carbon dioxide Temperature change in the last 50 years 2011-2021 average vs 1956-1976 baseline (°C) -1.0 -0.5 -0.2° +0.2 +0.5° +1.0° +2.0° +4.0° O 4 pairs of nonbonding electrons missing O 1 pair of nonbonding electrons missing O2 pairs of nonbonding electrons missing O 3 pairs of nonbonding electrons missingarrow_forward5. For the chemical reaction below (please note, this is the same as CH4 + Br2 → CH3Br + HBr; the Br2 over the arrow is a reactant. Let me know if you have any questions about this): a. How many non-polar and polar bonds are in the reactants? b. How many non-polar and polar bonds are in the products? c. What is the change in enthalpy (AH) for this reaction (positive or negative)? What is the evidence for your response? d. What is the change in entropy (AS) for this reaction (positive or negative)? What is your evidence for your response? e. Is this reaction exergonic (spontaneous) or endergonic (nonspontaneous)? f. Is the carbon in this reaction being reduced or oxidized? What evidence do you have for your claim? H H-CH- H Br₂ hv H H-C-Br + -Br + HBr Harrow_forward
- 10. You're preparing for a camping trip. you see two different stoves you can pack for your trip to do all your cooking. Which fuel would you prefer to carry? One stove uses fuel propane. The other stove uses naphtha (hexane) fuel. Start by writing a balanced combustion equation for both of these reactions. Use either standard enthalpies of formation or bond energies to determine the enthalpy changes for the combustion of these two fuels. Then suggest which stove, the one that uses propane or the one that uses naphtha, would you recommend to pack for your camping trip? Explain. (You may need more space for your response).arrow_forwardBond Type C - H 0=0 O-H C=O Energy (kJ/mol) 413 495 463 799 1. Using the bond energies given in the table, determine the total bond energy of the reactant molecules, 1 mole of CH4 and 2 moles of O2, in kilojoules (kJ). Upload an image of your response by clicking "Upload files" or by dragging and dropping your file into the box. Or use your device's camera to take a photo of your work by clicking the camera icon. ↑ T m + Upload files Supported file formats: PDF, JPG, PNG, RTF, TXT, ZIP, Word, Excel, Publisher, Open Office 0/3 File Limitarrow_forward2. Use equations (1) to (4) to calculate the enthalpy change for the reaction represented by equation (5). (1) P. (s) + 6CI2 (g) → (2) Pa (s) +5 0 (g) → 4 P,O10 (g). (3) PCI3 (g) +Cl2 (g) → PCI, (g) (4) PCI3 (g) +¬O2 (g) → POCI; (g) (5) P010 (s)+6 PCI5 (g) 4 PCI3 (g) AH =-1226 kJ AH = 2967 kJ AH = 84 kJ ΔΗ - - 286 kJ 10 POCI3 (g)arrow_forward
- 1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJarrow_forwardHess's Law is a useful way for chemists to predict the enthalpy change for a reaction. Use your understanding of energy changes to explain how Hess's Law works. Use the following example as part of your explanation (but you don't have to solve it!). 8. How can Hess's law be applied to determine the enthalpy change for the decomposition of potassium bicarbonate: 2 KHCO, (9) – K,CO; (s) + H,O () + CO2 (2) AH = -963 kJ (1) K (9) + ½ H, (e) Ce +0, (9)→ KHCO; (5) 2 (g) AH = -1150 kJ (2) 2K (9) + C + 02 (e) → K,C03 (6) AH = -242 kJ (3) H2() + ½ O2() H,O (g) AH = -394 kJ (4) C (6)+02 (g) - CO2 (2)arrow_forward[References] Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and wate are the products. Using the enthalpies of combustion for C,H2 (-1300. kJ/mol), C2Hs (-1560. kJ/mol), and H2 (-286 kJ/mol), calculate AH for the reaction C2H2 (g) + 2H2 (g) C2H (g) AH= kJ Submit Answer Try Another Version 1 item attempt remaining Previous Next 8:33 P 12/5/20 a S 0 門 thingarrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning