Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25 °C, diamond changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. Determine AHxn for (diamond) C(graphite) with equations from the following list: (1) CO₂ (g) C(diamond) + 0₂ (2) 2CO₂(g) → 2CO(g) + O₂(g) (3) CO₂(g) C(graphite) + O₂(g) (4) 2CO(g) C(graphite) + CO₂(g) ΔΗ → overall kJ Be sure your answer has the correct number of significant figures. ☐x10 ΔΗ=395.4 kJ X ΔΗ=566.0 kJ ΔΗ=393.5 kJ AH=-172.5 kJ

Diamond and graphite are two crystalline forms of carbon. At 1 atm and 25 °C, diamond changes to graphite so slowly that the enthalpy change of the process must be obtained indirectly. Determine AHxn for (diamond) C(graphite) with equations from the following list: (1) CO₂ (g) C(diamond) + 0₂ (2) 2CO₂(g) → 2CO(g) + O₂(g) (3) CO₂(g) C(graphite) + O₂(g) (4) 2CO(g) C(graphite) + CO₂(g) ΔΗ → overall kJ Be sure your answer has the correct number of significant figures. ☐x10 ΔΗ=395.4 kJ X ΔΗ=566.0 kJ ΔΗ=393.5 kJ AH=-172.5 kJ

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

4
Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) → H,0(g) AH1 = -241.8 kJ 2) X(s) + 2 Cl,(g) → XCl,(s) AH2 = +475.9 kJ 3) H,(g) + CL,(g) HCl(g) АНз 3 —92.3 kJ → 4) X(s) + O,(g) –→ XO,(s) AH4 = -748.7 kJ 5) Н, О(2) — н,00) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2H,О() — ХО,(8) + 4 HCI(g)
Ethanol can be made from the fermentation of crops and has been used as a fuel additive to gasoline. C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g)C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Part B Calculate ΔrH∘ (The standard enthalpy of formation of liquid ethanol is −277.6 kJmol−1, of gaseous carbon dioxide is −393.5 kJmol−1, and of gaseous water is −241.8 kJmol−1.) Express your answer in kilojoules per mole to one decimal place.
(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.
A simple method for the laboratory preparation of hydrogen involves reaction of zinc with hydrochloric acid;Zn(s) + 2 HCl(aq) → ZnCl 2(aq) + H 2(g) ΔH = -152.5 kJ How much heat in kilojoules is evolved if a total of 1094 mL of H 2 was collected over water at 28.00 ° C and an atmospheric pressure of 275.7 mm Hg. The partial pressure of water at this temperature is 28.35 mm Hg? Assume heat evolved is directly proportional to the moles produced.
12.00 g of Compound with molecular formula C4h8 are burned in a constant-pressure calorimeter containing 15.00 kg of water at 25 °C. The temperature of the water is observed to rise by 8.603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. calorimeter itself.)
Determine the enthalpy for the production of 5.0 g of H2 in the following target equation, making use of the known equations given below. CH4 (g) + NH3 (g) → HCN(g) + 3H2 (g) Using the following given equations: N2 (g)+3H2 (g) → 2NH3 (g) ΔH=− 91.8kJ C(s)+2H2 (g) → CH4 (g) ΔH=− 74.9kJ H2(g) + 2C(s) + N2 (g) → 2HCN(g) ΔH= + 270.3 kJ
A sample of steam with a mass of 0.506 g at a temperature of 100 ∘C condenses into an insulated container holding 4.20 g of water at 3.0 ∘C . For water, ΔH∘vap=40.7kJ/mol and Cwater=4.18J/(g⋅∘C) .
The industrial synthesis of chloroform by the reaction of methane with Cl2 is carried out according to the following reaction equation: CH4 (g) + Cl2 (g) → CHCl3 (l) + HCl (g) Using the thermodynamic data provided, calculate DHo (in Kj/mol) for this reaction.
Consider the following 2 reactions: 2A+B>2C -483.6KJ 3B>2D 284.6KJ determine the enthalpy change for the process: 3A+D>3C
PCI5(s) can be prepared by the reaction PCI3(1) + Cl2(g) - PCI5(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCI5(s) by the above reaction, given the following data. P4(s) + 6 Cl2(g) - 4 PC|3(1) AH° = -1280 kJ per mole of P4(s) %3D P4(s) + 10 Cl2(g) – 4 PCI5(s) ΔΗ AH° = -1774 kJ per mole of P4(s) +59.3 -59.3 +124 -124 -258
Hess's Law Given the following data: 4C(s) + 3H2(g) + 1/2O2(g) → HCOC(CH2)(CH3)(l) ΔH°=-139.0 kJ CH3CH2OH(l) + 1/2O2(g) → CH3CHO(l) + H2O(l) ΔH°=-204.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:2CH3CHO(l) → HCOC(CH2)(CH3)(l) + H2O(l)