Please correct answer and don't use hand rating 4งStarting with the Building problem from Module 5...A hydrocarbon is combusted in a controlled environment with pure oxygen. Upon combustion, a sample yielded 72.1g H2O and 176.28gCO₂. The molar mass of this unknown compound is about 28 g/molDraw the Lewis structure of this compound.What is the electron geometry around the carbon atom(s)?Write the balanced combustion equation.If 60.0g of the hydrocarbon and 200.0g of oxygen gas are introduced in the chamber. What is the percent yield of CO₂?What is the standard enthalpy of formation for this reaction?⚫ What is the heat generated from the reaction conditions as identified above?Da

1. Identifying the Hydrocarbon and Drawing its Lewis StructureWe are given:The sample produced 72.1…

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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 26Q

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Use a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.
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hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?
Estimate ΔrH° for forming 2 mol ammonia from molecular nitrogen and molecular hydrogen. Is this reaction exothermic or endothermic?
The molecular structure shown is of one form of glucose, C6H12O6 Glucose can be oxidized to carbon dioxide and water according to the equation C6H12O6(S) + 6 O2(g)6 CO2(g) + 6 H2O(g) (a) Using the method described in Section 6-6a for estimating enthalpy changes from bond energies, estimate rH for the oxidation of this form of glucose. Make a list of all bonds broken and all bonds formed in this process. (b) Compare your result with the experimental value of 2816 kJ/mol for combustion of glucose. Why might there be a difference between this value and the one you calculated in part (a)?
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1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJ
a) Define the term average bond enthalpy. b) Determine a value for the hydrogenation of propene. Thank you!
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Consider an internal combustion engine like that used in automobiles. The most common fuel used here is gasoline which is a mixture of hydrocarbons, and an octane rating is given for standardization. Therefore, we will approximate gasoline as being composed of the hydrocarbon, octane, C8H18. Another fuel that is common in racing applications is nitromethane, CH3NO2, used in top fuel dragsters. Let’s consider the combustion of each fuel with oxygen in an internal combustion engine. Let the 8-cylinder engine displacement be 500 in3 total. GOAL: Determine and compare the maximum enthalpy of reaction, ∆Ho rxn, for the combustion of both octane and nitromethane in a single cylinder of the engine. This means determine the maximum amount of fuel that can burn in the cylinder filled with 1 atm of air and the amount of heat that reaction would generate. Here are some suggested steps to guide you along. You will have to look up some data in your book or on the internet. 1. Write a balanced…

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