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.
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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)?
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
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
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?
8 Consider the combustion of liquid CH in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of CH is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.630 °C. 8 If-4789 J of heat was produced from the combustion of 0.001561 moles of C₂H₂, what is the enthalpy change (in kJ/mol) for the 8⁹ combustion of CH?
Use the bond energies in the table to estimate the enthalpy of reaction for the oxidation of hydrogen sulfide 2 H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O (g) Bond H—S O=O S=O S—O O—H Energy (kJ/mol) 347 498 523 87 463

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