Ethene (C₂H4), at 25 °C and 1 atm, is burned with 300% excess air at 25 °C and 1 atm. Assume that this reaction takes place adiabatically at 25 °C and that the products leave at25 °C and 1 atm. Use the PG mixture model. Assume cp to be uniform at 1.005 kJ/kg-K.Part ADetermine the irreversibility of the process.Express your answer to five significant figures.a CTemplates Symbols stope/Displacement Vector undo redo reset keyboard shortcutsAds 'help'% ISubmit Request AnswerkJkg

The combustion reaction means the burning of any substance in presence of oxygen to form carbon…

Ethene (C₂H₂), at 25 °C and 1 atm, is burned with 300% excess air at 25 °C and 1 atm. Assume that this reaction takes place adiabatically at 25 °C and that the products leave at 25 °C and 1 atm. Use the PG mixture model. Assume cp to be uniform at 1.005 kJ/kg.K.

Ethene (C₂H₂), at 25 °C and 1 atm, is burned with 300% excess air at 25 °C and 1 atm. Assume that this reaction takes place adiabatically at 25 °C and that the products leave at 25 °C and 1 atm. Use the PG mixture model. Assume cp to be uniform at 1.005 kJ/kg.K.

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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If you need to reverse the following reaction in order for it to be an intermediate reaction in a Hess's law problem, what would be the final value for the enthalpy of reaction you use for this intermediate reaction? C2H4 + 3 02→2 CO2 + 2 H20, AH = -1410 kJ O A. 2820 kJ O B. -1410 kJ O C. 1410 kJ O D. -2820 kJ
Given the standard heats of formation for the following compounds, calculate AH of the reaction at 298". 12NH 210e SHNO30 4NO) + 14HO 459 -133.9 91.3 -2418 0-4650 O-2259 4270kJ O 3540
PART 4 PLEASE
DATA AND CALCULATIONS Reaction 2 Reaction 3 Reaction 1 (no solid NaoH) 2154 100. 154 a8.5 Mass of NaOH solid 100 t00.061 34.8 d1.9 Mass (total) of solution 6. 9. 6. °C 33.3 °C Final temperature, T2 °C av. °C al. 7 Initial temperature, T °C °C CALCULATIONS temperature change, AT 6.7 °C la. 9 °C I1.6 °C kJ -5395.489 k-4848.8 -ag04.913 a804.913 k- $395.499 KJ|-4848.8 Heat, q kJ ΔΗ k) Moles of NaOH 0.054 mol 0.0515 0.05 mol mol AH/mol -51,942.83k)/mol-104 96.70kJ/mol-96 976 kJ/mol Experimental value kJ/mol Accepted value k)/mol Percent error %
A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g•°C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.
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Jorge is trying to classify the reaction represented by the graph below and calculate the change in energy, AH for it. 250 ***** . ******.... 200 ****** PE 150 (kJ) 100 ...... 50 ....
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