One method for making ethanol, C₂H5OH, involves the gas-phase hydration of ethylene, C₂H4: Estimate AH for this reaction from the given average bond dissociation energies. Set your reaction up as follows: C₂H₂ + H₂O-C₂H₂OH Bond D, kJ/mol C=C 615 410 350 C-H C-C C-0 O-H -35 350 460 Your answer is correct. Part 2 of 2 2 16 % X ala 19 What is the amount of energy, in k3, changed upon hydration of 63.1 10 11.9 %

One method for making ethanol, C₂H5OH, involves the gas-phase hydration of ethylene, C₂H4: Estimate AH for this reaction from the given average bond dissociation energies. Set your reaction up as follows: C₂H₂ + H₂O-C₂H₂OH Bond D, kJ/mol C=C 615 410 350 C-H C-C C-0 O-H -35 350 460 Your answer is correct. Part 2 of 2 2 16 % X ala 19 What is the amount of energy, in k3, changed upon hydration of 63.1 10 11.9 %

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 ΔH for the target reaction below using the three equations listed. Rewrite the three equations so that they add to give the reaction below Target: CS2(l) + 3O2(g) --> CO2(g) + 2SO2(g) ΔH = ? C(s) + O2(g) --> CO2(g) ΔH = -393.5 kJ S(s) + O2(g) --> SO2(g) ΔH = -296.8 kJ C(s) + 2S(s) --> CS2(l) ΔH = 87.9 kJ Enter ΔH for the top equation in Kj. (Your answer should have one digit after the decimal)
Using bond enthalpies in the table, estimate AH for the following gas-phase reactions. Average Bond Enthalpies (kJ/mol) Single Bonds C-H C-C C-N C-O C-F C-Cl C-Br C-I C-S 413 |N-H 348 |N-N 293 N-O 358 |N-F 485 |N-Cl 328 N-Br 243 276 240 259 CH–C1 242 193 Br-Br Multiple Bonds C=C C=C C=N C=N 614 839 615 391 O-H 0-0 163 201 O-F 272 O-Cl 200 O-I 201 463 146 190 203 234 339 H-H S-H 436 S-F 567 S-Cl 327 253 H-F H-Cl 431 S-Br 218 H-Br 366 S-S 266 H-I 299 |N=N 418 0=0 |N=N 941 |N=O 607 495 Part C Estimate AH for the reaction. Express your answer using one significant figure. AH = Submit —| ΑΣΦ Provide Feedback H H-N-N-H+CI-CI-2 H-N-CI -H+C₁_a_ Previous Answers Request Answer HH X Incorrect; Try Again; 3 attempts remaining ? kJ
Using the standard formation enthalpies that follow, calculate the standard enthalpy change for this reaction. A,H° = cog) + H,O(1) –→ CO2(g) + H2(g) AH° (kJ/mol) kJ Species Co(g) -110.5 H201) -285.8 CO2(g) -393.5
A chemist measures the enthalpy change AH during the following reaction: P4(s) + 6 Cl₂(g) →4 PC1₂(g) AH-1148. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction PC₁₂ (9) → 4PCL, (g) P₁(s) + 2C₁₂ (9) P₁ (s) + 6Cl₂ (g) P₁ (s) + C₁₂(g) → PCI, (g) ΔΗ [] kJ KJ kJ x10 X
You are given the following average bond energies:H-H 436 kJ/molH-X 431 kJ/molH-C 414 kJ/molC-X 339 kJ/molX-X 243 kJ/molBalance the following chemical reaction and compute the estimated heat of reaction using the values above.CH4(g) + X2(g) → CH1X3(g) + HX (g)
Using the given molar enthalpies of formation, determine the change in enthalpy for the combustion of 1 mole of methanol. , AH°; CH3OH (4) =- 238.6 kJ/mol AH°; CO2 (g) = - 110.5 kJ/mol AH°; H2O (g) = – 241.8 kJ/mol 3 CH3OH (e) +02 (g) → CO2 (g) + 2H2O (g)
Use the bond energies provided to estimate AH°rxn for the reaction below. XeF6 AH°rxn = ? Bond Xe-F F-F XeF2+2F2 Bond Energy (kl/mol) 147 159 O-270 kJ +159 kJ -660 kJ +176 kJ -429 kJ K
Consider the reaction. 2Fe2O3⟶4Fe+3O2Δ?∘rxn=+824.2 kJ2Fe2O3⟶4Fe+3O2ΔHrxn°=+824.2 kJ The formation of 75.0 g75.0 g of O2 results in the absorption of 1930 kJ1930 kJ of heat. the absorption of 20600 kJ20600 kJ of heat. the release of 20600 kJ20600 kJ of heat. the release of 644 kJ644 kJ of heat. the release of 1930 kJ1930 kJ of heat. the absorption of 644 kJ644 kJ of heat.
The reaction we performed was: Na(s) + H2O(l) NaOH(aq) + 1/2H2(g) qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is: 0 = qsystem = qreaction + qwater qreaction = -qwater qreaction = -mwater*Cwater*Twater The data from the demonstration was: (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g What is Tfinal in centigrade?
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The thermite reaction is a very exothermic reaction; it has been used to produce liquid iron for welding. A mixture of 2 mol of powdered aluminum metal and 1 mol of iron(III) oxide yields liquid iron and solid aluminum oxide. How many grams of the mixture are needed to produce 219 k) of heat? Data: AH;(Al(s)) = 0 kJ/mol AH (Fe,O3 (s)) = -825.5 kJ/mol AH (Fe(1)) = 12.4 kJ/mol AH;(Al2O3 (s)) = -1675.7 kJ/mol
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