help me asap pls that is less than 30 mins with number 19. i'll give you an upvote after! 19Calculate AH° and AE° for the following reactions at 25 °C. Use standard enthalpies of formation from the table below. Round youranswers to four significant digits.SubstanceANO mol-)SubstanceAN N mol-)-393.5GH,)(CH,),COU)H,O()HCK)226.75NHg)-46.19-248.1NH,CIG)-3154-241.881.57-92.30(a) 2C2H2(g) + 502(8) – 4CO2(3) + 2H2O(g)AH° =kJAE =kJ(b) C,H;g) + SN;OG) –- 200;g) + H;OG) + 5N;G)AH-kJAE-kJ(c) NH,Cs) - NH3(s) + HCIg)AH -kJAE° -kJ(d) (CH3)2COU) + 4O2(3) - 3CO2(g) + 3H2O(G)AH-kJAE-kJ

As per our guidelines we can only solve first three sub-parts. Please resubmit the other questions…

19 Calculate AH" and AE" for the following reactions at 25 °C. Use standard enthalpies of formation from the ta answers to four significant digits. Snce AN Stance -393.5 226.75 NHg) NH,C) -46.19 (CH,,COU) H,O HO -248.1 -3154 -241.8 1.57 -92.30 (a) 2C;H2le) + 5O;lg) → 4CO;lg) + 2H;Olg) AH kJ AE kJ (c) NH,Cs) - NH(g) + HCg) AH-

19 Calculate AH" and AE" for the following reactions at 25 °C. Use standard enthalpies of formation from the ta answers to four significant digits. Snce AN Stance -393.5 226.75 NHg) NH,C) -46.19 (CH,,COU) H,O HO -248.1 -3154 -241.8 1.57 -92.30 (a) 2C;H2le) + 5O;lg) → 4CO;lg) + 2H;Olg) AH kJ AE kJ (c) NH,Cs) - NH(g) + HCg) AH-

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 9RQ: Define the standard enthalpy of formation. What are standard states for elements and for compounds?...

See similar textbooks

Similar questions

When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Natural gas is mostly CH4. When it burns, the chemical reaction is CH4 g 2O2 g CO2 g 2H2O g The H of combustion of one mole of CH4 at 25.0 C is -890.9 kJ. Calculate q, w, and U under these conditions, assuming an external pressure of 1.07 atm.
For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
Define the standard enthalpy of formation. What are standard states for elements and for compounds? Using Hess's law, illustrate why the formula Hreaction=npHf(products)nfHf(reactants) works to calculate H for a reaction.
Use standard entropies and heats of formation to calculate G f at 25C for (a) cadmium(II) chloride (s). (b) methyl alcohol, CH3OH(l). (c) copper(I) sulfide (s).
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
Methane can be produced from CO and H2.The process might be done in two steps, as shown below, with each step carried out in a separate reaction vessel within the production plant. Reaction 1 CO(g)+2H2(g)CH3OH(l) S = -532 J/K Reaction 2 CH3OH(l)CH4(g)+12O2(g) S= +162 J/K NOTE: You should be able to work this problem without using any additional tabulated data. (a) Calculate H for reaction 1. (b) Calculate Gf for CO(g). (c) Calculate S° for O2(g). (d) At what temperatures is reaction 1 spontaneous? (e) Suggest a reason why these two steps would need to be carried out separately. Substance Hf (kJ mol-1) Gf (kJ mol-1) S (J mol-1 K-1) CO(s) -110.5 197.674 CH3OH( l ) -238.7 -166.4 126.8 CH4(g) -74.8 186.2
A 2.50-mol sample of gas is compressed isothermally from 20.0 L to 5.00 L under a constant external pressure of 10.0 atm. Calculate w, q, U, and H for the process.
Identify the sign of the work when a fuel-oxygen mixture (the system) burns, propelling an automobile (part of the surroundings).