**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]

Answered: Image /qna-images/answer/ec7f8f84-7540-4a17-9dc9-5b54699e4c7f.jpg

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

See similar textbooks

Similar questions

Help me
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
powo 72 3. Calculate the heat of combustion (kJ) of propane, C3H8 using the listed standard enthalpy of reaction data: C3H8(g) + 5 O2(g) →3 CO2(g) + 4 H₂O(g) AH° = -103.8 kJ AH = -393.5 kJ AHO = -241.8 kJ 3 C(s) + 4 H₂(g) →→ C3H8(g) C(s) + O2(g) → CO2(g) H₂(g) + 1/2 O2(g) → H₂O(g) 4. Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N₂(g) + 5 O₂(g) →2 N₂O5(g) AHO=-571.6 kJ AH°= -73.7 kJ AH°=-348.2 kJ (24 2 H₂(g) + O2(g) → 2 H₂O(1) N₂Os(g) + H₂O(1)→ 2 HNO3(1) N2(g) + 3 O2(g) + H₂(g) → 2 HNO3(1) HA
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
q= cAT = msAT = ms(Tinal – Tiniia) AHΧΣn, ΧΑΡ(prod)] - Σn, ΧΔΗ (react)] 1. The enthalpy of which of the following reactions would not be the enthalpy of formation of the product? a) 1/2 H,(g) + 1/2 Br:(1) ---> HBr(g) c) H,O(1) + SO,(1) ---> H,SO,(1) b) H.(g) + 1/2 O,(g) H;O(1) d) Ca(s) + 1/2 O:(g) ---> CaO(s) --->
Combustion of methane. Refer to the second question in the attached image. Apparently with one mole of methane combustion the pressure and volume are different for gasses in the reaction.
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
Sucrose, C12 H22011, is common table sugar. The enthalpy change at 25°C and 1 atm for the complete burning of 2 mol of sucrose in oxygen to give CO2(9) and H2O(1) is - 1.128 x 10* k. From this and from data given below: AH (H2O(1) = -285.8 kJ/mol AH (CO2(9)) = -393.5 kJ/mol AH (O2(9) = 0 kJ/mol Calculate the standard enthalpy of formation of sucrose. AH; =| K/mol
4- Use Hess's law to calculate the enthalpy change (in kJ/mol) of Alanine oxidation (ΔH1) using the below individual steps. C3H7NO2(s) + 3O2(g) → 5 2 CO2(g) + 5 2 H2O(l) +1 2 (H2N)C=O(s) ΔH1 =?? (H2N)C=O(s) + 3 2 O2(g)→CO2(g) + 2 H2O(l) + N2(g) ΔH2 = -632 KJ/mol C3H7NO2(s) + 15 4 O2(g) → 3 CO2(g) + 7 2 H2O(l) + 1 2 N2(g) ΔH3 = -1577 KJ/mol
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
when octane (C8H18) is burned under standard conditions, the enthalpy of combustion is -5698.34KJ / mol. Using the information provided. what is the heat of formation of octane?