3. Calculate the heat of reaction (AHr, To) and adiabatic combustion temperature (Tad)of a fuel mixture (50 mol% octane + 50 mol% n-butane) burning with air at =0.8, as following→C8H18 (g) + C4H10(g) +x (O2 + 3.76N2) aCO2 + bH2O + CO2 + dN₂

To calculate the heat of reaction (ΔH°) and adiabatic combustion temperature (Tad) of the given fuel…

Answered: 3. Calculate the heat of reaction (AHr,…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the change of enthalpy for the reaction 2AI (s) + 3C12 (g) --> 2AICI3 (s) from the following reactions: Reaction 1: 2AI (s) + 6HCI (aq) --> 2AICI3 (aq) + 3H2 (g) Change in enthalpy: -1049 kJ Reaction 2: HCI (g) --> HCI (aq) Change in enthalpy: -74.8 kJ/mol Reaction 3: H2 (g) + Cl2 (g) --> 2HCI (g) Change in enthalpy: -1845. kļ/mol Reaction 4: AICI3 (s) --> AICI3 (aq) Change in enthalpy: -323. kJ/mol Include the following: • The numerical answer with correct units. • State which reactions, if any, you had to "Flip". • State which reactions you had to multiply, if any, to get the correct amount of the compound.
V:OY IA %YA N& 令 l PNG.9 → حداد H.W) calculate AçH° (500 K) for methane by using the data given on the temperature dependence of heat capacities. CH4(g)+2O2(g)→CO2(g)+2H2O(g) AÇH° (298 K) -891 kJ Cp,m(CO2) = 44.22 + 8.79 × 10-37 - 8.62 × 105 T2 Cp.m(H2O) = 75.29 + 0 + 0 Cp,m(O2) = 29.96 + 4.18 × 10-37 1.67 × 105 T2 Cp,m(CH4) = 35.31
The equation I found for 2a was: C3H6 + 9/2 O2 ----> 3CO2 +3H2O
(d) The enthalpy change for the reaction (A,Hº) of ethyne (C,H,) is -2511.6 kJ. i. Write a balance equation for the combustion of ethyne. ii. Determine the enthalpy of formation A¡Hº of ethyne given the following: A¢H° CO2 = -393-5 kJ mol" A¡Hº H2O_ = -241.8 kJ mol" A¡H° O2 = 0.00 kJ mol-1 %3D
8) Kirchhoff's Law Calculate the reaction enthalpy for the following reaction (ARH° = - 282.98 kJ mol¹¹) at a temperature of 400 °C: CO+0.502 → CO₂ In your calculations, consider the temperature-dependency of the molar heat capacities as follows: Cp (CO) = (21.75 +0.064 T-4.1.10-5T2)Jmol-¹K-1 Cp(O2) = (27.96 +0.004 T-1.7 10-7T²)Jmol¯¹K−¹ Cp (CO2)=(27.63 +0.005 T)Jmol-1K-1
Q5 (i) Draw an energy cycle and use the Standard Enthalpies of combustion values in the table below to calculate the 10(g)* enthalpy of formation of butane, C4H₁09). Explain how the value obtained here might be different from the value obtained using calorimetry. (Show working as this question will be assessed using grade descriptors 1, 3 & 7) Substance Enthalpy of Combustion/kJ mol-¹ -394 -286 -2876 C(s) H2(g) CH10(9)
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…
Please help with D & E

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3. Calculate the heat of reaction (AHr, To) and adiabatic combustion temperature (Tad) of a fuel mixture (50 mol% octane + 50 mol% n-butane) burning with air at = 0.8, as following → C8H18 (g) + C4H10(g) +x (O2 + 3.76N2) aCO2 + bH2O + CO2 + dN₂