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 & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 88PS

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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.
hat is meant by the term driving forces? Why are mailer spread and energy spread considered to be driving forces?
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
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)?
Given the listed average bond energies (BE), calculate the enthalpy change for the production of one mole of methanol (CH3OH) by the following reaction. (There are two C=O double bonds in CO2) CO2(g) + 3 H2(g) → CH3OH(g) + H2O(g) B.E.C–O = 300 kJ/mol B.E.C=O = 700 kJ/mol B.E.H–H = 450 kJ/mol B.E.H–O = 500 kJ/mol B.E.H–C = 400 kJ/mol Select one: a. -250 kJ b. -950 kJ c. 950 kJ d. 50 kJ e. 250 kJ
210 6. Calculate enthalpy change of the reaction using enthalpy of formation values. Hint: Used Balanced equation. - C3H8(g) + O₂ (g) → AH values in kJ/mol CO₂(g) + H₂O(1) C3H8(g) = -103.8; CO₂ (g) = -393.5; H₂O (1) = -285.8 Slonel'i 34 140m² p vrl=3 odtyd enab how to £25031 odi to ondo verons lamotri Lar
Bond Type C - H 0=0 O-H C=O Energy (kJ/mol) 413 495 463 799 1. Using the bond energies given in the table, determine the total bond energy of the reactant molecules, 1 mole of CH4 and 2 moles of O2, in kilojoules (kJ). Upload an image of your response by clicking "Upload files" or by dragging and dropping your file into the box. Or use your device's camera to take a photo of your work by clicking the camera icon. ↑ T m + Upload files Supported file formats: PDF, JPG, PNG, RTF, TXT, ZIP, Word, Excel, Publisher, Open Office 0/3 File Limit
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
8. Determine the enthalpy for the following reaction, given AH, (NH3(g)) = -46.1 kJ/mol, AH; (NO(g)) = +90.3 kJ/mol, and AH (H20(g)) = -241.8 kJ/mol. %3D 4NH3(g) + 502(g) → 4NO(g) + 6H20(g) AHn = ? kJ %3D a. -1274 kJ/mol d. -905.2 kJ/mol b. -1,996 kJ/mol +1,274 kJ/mol е. -105.4 kJ/mol с.
What is the enthalpy for the reaction?

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