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

Oluşum Entalpileri (kJ/mol) C3HS (g)-103.8 0, (8) CO, (g) H,O (s) -393.5 -285.8 Using the table above, find the enthalpy change (AH) of the combustion reaction shown below for 1 mole of propane (C3H8). C;H3 (g) + 502 (g) 3CO2 (g) +4H,O (s) O A) -2427.5 kJ O B) +575.5 OC) -783.1 kJ O D) +2427.5 kJ O E) -2219.9 kJ

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

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…

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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

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.

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

Part A Calculate the enthalpy change when 5 L of liquid NH3 is burned in air to give N2 (9) and H,O(g). Express your answer using two significant figures. AH° - -7.0x10* kJ Submit Previous Answers v Correct Part B How does this compare with AH for the complete combustion of 1 L of liquid methanol, CH3 OH(1)? For CH,OH(1), the density at 25 °C is 0.792 g/cm', and AH; equals -239 kJ/mol. Essay answers are limited to about 500 words (3800 characters maximum, including spaces). 3800 Character(s) remaining Submit Request Answer Course Home Ammonia (NH3) boils at -33° C; at this temperature it has a density of 0.81 g/cm. The enthalpy of formation of NH3 (g) is -46.2 kJ/mol, and the enthalpy of vaporization of NH3 (1) is 23.2 kJ/mol.