**Calculate the Enthalpy of Reaction for the Combustion Reaction**Calculate the enthalpy of reaction for the combustion reaction (in kJ/mol) shown below. Enter your answer without units.\[ \text{Structural Representation of Ethene Combustion} \]\( \text{CH}_3\text{CH}_2\text{OH} + 5 \text{O} \equiv \text{O} \longrightarrow 4 \text{O} = \text{C} = \text{O} + 4 \text{H}_2\text{O} \)**Bond Energies Table:**| Bond | Average Bond Energy (kJ/mol) ||------|------------------------------|| H–H | 436 || H–C | 414 || H–O | 464 || C–C | 347 || C=C | 611 || C–O | 360 || C=O | 799 || O=O | 498 |**Instructions**- Analyze the given reaction by identifying bonds broken and bonds formed.- Use the bond energies provided in the table to calculate the overall enthalpy change. **Note:** If you cannot see the images above, [then click here](#).[Space for Answer]

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Calculate the enthalpy of reaction for the combustion reaction (in kJ/mol) shown below. Enter your answer without units. H H 4 0=c=o + 4 H-0-H Н-С—С C C-0-H + 5 0=0 H H Average Bond Energy Bond (kJ/mol) H-H 436 H-C 414 H-O 464 C-C 347 C=C 611 C-0 360 C=O 799 0-0 142 O=0 498 If you cannot see the images above,then click here

Calculate the enthalpy of reaction for the combustion reaction (in kJ/mol) shown below. Enter your answer without units. H H 4 0=c=o + 4 H-0-H Н-С—С C C-0-H + 5 0=0 H H Average Bond Energy Bond (kJ/mol) H-H 436 H-C 414 H-O 464 C-C 347 C=C 611 C-0 360 C=O 799 0-0 142 O=0 498 If you cannot see the images above,then click here

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.94PAE

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tml?ClassID=543616615# Calculate the enthalpy, in kJ/mol, for the combustion of the hydrocarbon from the data from the previous steps. 9cal = 6191.78 J n= 0.0019243682 mol AH = [ ? ] kJ/mol Enter either a + or - sign AND the magnitude. Give your answer to three significant figures. AH (kJ/mol) Enter
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Esc ||| = OTHERMOCHEMISTRY A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). Calculating heat of reaction from bomb calorimetry data First, a 5.000 g tablet of benzoic acid (C6H,CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 16.00 °C to 38.96 °C over a time of 9.2 minutes. 2 4. Next, 5.730 g of acetaldehyde (C₂H₂O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 42.19 °C. 84°F Sunny Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: FI Explanation Is this reaction exothermic, endothermic, or neither? 4- F₂ Check 2C₂H4O(g) + 50₂(g) 4CO₂(g) + 4H₂O(g) Be sure any of your answers that are…
O Macmillan Learning For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. 18⁹ 18 C8H₁8 (g) + 25/ 02(g) 8 CO₂(g) + 9 H₂O(g) 2 AH; = ΔΗ AH ixn = -5108.7 kJ/mol What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? Standard enthalpy of formation values can be found in this table of thermodynamic values. 8 18 kJ/mol
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Please answer this with in 30 mins ! I will upvote !
Мо Peer Leader: Date: Name: calculation and follow significant figure rules. _CH18(g) + O2(g) → CO2(g) + _H;O(1) H2O(1) > AH°pxn = -10940 kJ/mol CO:(g) AH°F = -393.5 kJ/mol %3D H¿O(1) AH°f = -285.8 kJ/mol
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Calculate the enthalpy of combustion for kerosene. Assume that kerosene is C10H22(l) and that the products are CO2(g) and H2O(l). ΔH°f (C10H22(l)) = –249.6 kJ/mol ΔH°f (CO2(g)) = –393.5 kJ/mol ΔH°f (H2O(l)) = –285.8 kJ/mol Select one: a. –872.9 kJ/mol b. –5489.9 kJ/mol c. –429.7 kJ/mol d. –6829.2 kJ/mol