Show work please This image shows a multiple choice question related to energy values in kilojoules (kJ). The options listed appear to offer various energy changes, both positive and negative. Here are the choices given:1. \(-8,790\) kJ2. \(45,400\) kJ3. \(-45,400\) kJ4. \(-22,700\) kJ5. \(-9,090\) kJThere are no graphs or diagrams in the image, just a list of numerical options framed within a multiple choice format. Pentaborane B₅H₉(g) burns vigorously in O₂ to give B₂O₃(s) and H₂O(l). Calculate ΔH_rxn for the combustion of 5.00 mol of B₅H₉.- ΔH°f[B₂O₃(s)] = -1273.5 kJ/mol- ΔH°f[B₅H₉(g)] = 73.2 kJ/mol- ΔH°f[H₂O(l)] = -285.8 kJ/molMultiple Choice Options:- ○ -8,790 kJ- ○ 45,400 kJ- ○ -45,400 kJ- ○ -22,200 kJ(Note: The given question involves calculating the enthalpy change for the reaction using standard enthalpy of formation values. The task is to determine which of the options corresponds correctly to the combustion of 5.00 mol of B₅H₉.)

Given: ∆Hof[B2O3(s)] = -1273.5 kJ/mol ∆Hof[B5O9(s)] = 73.2 kJ/mol ∆Hof[H2O(l)] = -285.8 kJ/mol moles…

Pentaborane BgHg(s) burns vigorously in 02 to give B203ls) and H2O). Calculate AHoxn for the combustion of 5.00 mol of B5H9. AHB203ls))=-1273.5 kJimol AH(BSHgls= 73.2 k/mol AHH2O) =-285.8 k/mol Multiple Choice

Pentaborane BgHg(s) burns vigorously in 02 to give B203ls) and H2O). Calculate AHoxn for the combustion of 5.00 mol of B5H9. AHB203ls))=-1273.5 kJimol AH(BSHgls= 73.2 k/mol AHH2O) =-285.8 k/mol Multiple Choice

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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Question

Show work please

Pentaborane B₅H₉(g) burns vigorously in O₂ to give B₂O₃(s) and H₂O(l). Calculate ΔH_rxn for the combustion of 5.00 mol of B₅H₉.

- ΔH°f[B₂O₃(s)] = -1273.5 kJ/mol
- ΔH°f[B₅H₉(g)] = 73.2 kJ/mol
- ΔH°f[H₂O(l)] = -285.8 kJ/mol

Multiple Choice Options:
- ○ -8,790 kJ
- ○ 45,400 kJ
- ○ -45,400 kJ
- ○ -22,200 kJ

(Note: The given question involves calculating the enthalpy change for the reaction using standard enthalpy of formation values. The task is to determine which of the options corresponds correctly to the combustion of 5.00 mol of B₅H₉.)

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