Use the bond energies provided to calculate the reaction enthalpy (AH°rxn) for the reaction: C2H4(g) + H2(g) – C2H6(g). Clearly show your work in the space provided below. For full credit, clearly show all your work in the space below, report your answer with correct sig figs and units, and place a box around your final answer. Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 H-H 436

Use the bond energies provided to calculate the reaction enthalpy (AH°rxn) for the reaction: C2H4(g) + H2(g) – C2H6(g). Clearly show your work in the space provided below. For full credit, clearly show all your work in the space below, report your answer with correct sig figs and units, and place a box around your final answer. Bond Bond Energy (kJ/mol) C-C 347 C-H 414 C=C 611 H-H 436

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...

See similar textbooks

Similar questions

19
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)
In this problem you are going to determine the molarity of a strong acid solution by measuring the enthalpy change of the acid’s reaction with a base, which causes the temperature of the reaction mixture to go from 22.3 °C to 34.8 °C. You will have to look up values from your OpenStax text. A) What is the underlying reaction of every acid-base neutralization reaction? What is the enthalpy change of this reaction per mole of acid? B) You performed this acid-base neutralization reaction with 100.0 mL of 2.00 M sodium hydroxide (base) and 60.0 mL of your unknown strong acid. What is the total volume of your reaction mixture after you mix the two solutions together? (The base is in excess.)
Consider the following reaction: 2 AB + 3 CD2 - 2 AD3 + C3B2 Use the provided standard enthalpies of formation to calculate the standard enthalpy change (AH rxn) for this reaction. Compound AH f (kJ/mol) AB CD2 AD3 C3B2 -587.0 +48.4 -471.2 -639.2
Use the molar bond enthalpy data in the table to estimate Bond kJ - mol-1 Bond kJ - mol- the value of AHin for the equation. О-Н 464 C=N 890 0–0 142 N-H 390 NH, (g) + 20,(g) → HNO, (g) + H,O(g) С-О 351 N-O 201 The bonding in the molecules is shown. O=0 502 N=N 418 C=0 730 N=O 607 + С-С 347 F-F 155 C=C 615 Cl-CI 243 C=C 811 Br-Br 192 С-Н 414 Н-Н 435 С-F 439 Н-F 565 C-CI 331 H-CI 431 С-Br 276 Н-Br 368 С-N 293 H-S 364 C=N 615 S-S 225 Activate WinkJomol-
Acetylene, C₂H2, can be reacted with molecular hydrogen (H2) to produce ethylene, C₂H4, as shown below: H H H H-CC-H C=C H H H Use the bond energies in the table below to estimate AH for this reaction in kJ. Bond Bond Energy C=C 620 kJ/mol C-H 414 kJ/mol C=C 812 kJ/mol H-H 436 kJ/mol C-C 347 kJ/mol
(incorrect) Calculate the standard enthalpy of reaction for the following reaction using the appropriate standard enthalpies of formation AH [SiCl4 (g)] = -657.0 kJ/mol; Other relevant thermodynamic quantities can be found in the appendix at the end of the textbook. SiO₂ (s) + 4 HCI (g) → SiCl4 (g) + 2 H₂O(g) -104.2 kJ 104.2 kJ -137.2 kJ -139.3 kJ (Your answer) 139.3 kJ (Correct answer)
Cles [References] TUTOR Predicting Enthalpy of Reaction Using Bond Energies Use the References to access important values if needed for this question. Use average bond enthalpies (linked above) to calculate the enthalpy change for the following gas-phase reaction. 2H2(g) + O2(g) →→→2H2O(g) To analyze the reaction, first draw (on paper) Lewis structures for all reactant and product molecules. AHreaction Submit kl Show Approach Show Tutor Steps Submit Answer Try Another Version 10 item attempts remaining
a) Using the balanced equation and the data in the table below, calculate the theoretical enthalpy of combustion. Note: you will need to include the enthalpy of vaporisation for the liquid components which are also given. CH3OH() +1.502(g) → CO2(g) + 2H2O (1) Average Bond Enthalpies (kJ mol‍¹) C-H C-C C-O O=O C=O O-H Enthalpy of Vaporisation (kJ mol-¹) Methanol Water 412 348 358 496 743 463 35 41
What volume of 1.772 M BaCl2 is needed to obtain 123 g of BaCl2?
Substance AH (kJ/mol) MgCl2(aq) -785.1 kJ/mol HCl(aq) -167.2 kJ/mol Given the enthalpy of formation data in the table, what is the enthalpy of reaction for the reaction you performed in this lab? To calculate the enthalpy of reaction, use the following formula. AHrxn =ΣAH(products) - ΣAH; (reactants) Note that you will need the balanced chemical equation for the reaction performed in the lab. Also, note that AH; for the standard state elements is 0 kJ/mol. AHrxn = Is the calculated result simliar to the experimentally determined result? yes no kJ/mol
A chemist measures the enthalpy change AH during the following reaction: 2 KCl(s) + 30₂(g) →2 KClO3(s) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction 2 KCI(s) + O₂(g) →KCIO₂ (s) 6K CIO3 (s) 6KCI(s) + 90₂ (g) 2K CIO3(s) 2KCI(s) 2KCl(s) + + 30₂ (g) ΔΗ = 78. kJ ΔΗ เม Ок kJ kJ kJ x10 X Ś