Problem 19.70Methanol (CH3OH) can be made by the controlled oxidation ofmethane:CH4(g) + O2(g) → CH₂OH(g)Part ACalculate AHⒸ for this reaction. Use the following data: AH (CH₂OH(g))Express your answer in kilojoules to one decimal place.IV. ΑΣΦΔΗ -SubmitPart BAS =SubmitRequest AnswerPart C|VL]| ΑΣΦ 1Calculate ASfor this reaction. Use the following data: SP (CH3OH(g)) = 237.6 J/(mol-K), Sę (CH4(g)) = 186.3 J/(mol-K).S (O₂(g)) 205.15 J/(mol-K)Express your answer in joules per kelvin to one decimal place.Request AnswerO increasesIywvK ?O decreasesOstays the samekJ?Will AG for the reaction increase, decrease, or stay unchanged with increasing temperature?201.2 kJ/mol. AH? (CH4(g))J/K40 of 41Review | Constants | Periodic Table74.6 kJ/mol. AH (O₂(g)) = 0 kJ/mol. FPart DCalculate AG at 298 K.Express your answer in kilojoules to one decimal place.AGO =SubmitPart FV—| ΑΣΦPart E Complete previous part(s)Request AnswerSubmitIs there a temperature at which the reaction would be at equilibrium under standard conditions and that is low enough so that the compounds involved are likely to be stable?Match the items in the left column to the appropriate blanks in the sentences on the right.AG > 0attainableunattainable?AG <0AG=0kJRequest AnswerReset HelpThe reaction is at equilibrium when. To reach an equilibrium, the temperature of thesystem should be so high that the reactants and products are likely to decompose. Therefore,equilibrium is functionallyfor this reaction at standard conditions.

Answered: Image /qna-images/answer/862c4712-0493-4d22-9f77-8c7f88463e6d.jpg

Problem 19.70 Methanol (CH3OH) can be made by the controlled oxidation of methane: CH4 (8) + O₂(g) → CH₂OH(g) Part A Calculate AH® for this reaction. Use the following data: AH (CH₂OH(g)) Express your answer in kilojoules one decimal place. LIVE ΑΣΦ A AH° = Submit Part B AS" = Submit Request Answer Part C Calculate AS® for this reaction. Use the following data: Sp(CH₂OH(g)) = 237.6 J/(mol-K). Sp (CH4(g)) 186.3 J/(mol-K). S(O₂(g)) 205.15 J/(mol K). Express your answer in joules per kelvin to one decimal place. IVD ΑΣΦΑ Request Answer ? A & O increases O decreases Ostays the same kJ ? J/K Will AG for the reaction increase, decrease, or stay unchanged with increasing temperature? 40 of 41 Review | Constants | Periodic Table 201.2 kJ/mol. AH (CH.(g)) 74.6 kJ/mol. AH (O₂(g)) 0 kJ/mol. >

Problem 19.70 Methanol (CH3OH) can be made by the controlled oxidation of methane: CH4 (8) + O₂(g) → CH₂OH(g) Part A Calculate AH® for this reaction. Use the following data: AH (CH₂OH(g)) Express your answer in kilojoules one decimal place. LIVE ΑΣΦ A AH° = Submit Part B AS" = Submit Request Answer Part C Calculate AS® for this reaction. Use the following data: Sp(CH₂OH(g)) = 237.6 J/(mol-K). Sp (CH4(g)) 186.3 J/(mol-K). S(O₂(g)) 205.15 J/(mol K). Express your answer in joules per kelvin to one decimal place. IVD ΑΣΦΑ Request Answer ? A & O increases O decreases Ostays the same kJ ? J/K Will AG for the reaction increase, decrease, or stay unchanged with increasing temperature? 40 of 41 Review | Constants | Periodic Table 201.2 kJ/mol. AH (CH.(g)) 74.6 kJ/mol. AH (O₂(g)) 0 kJ/mol. >

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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2. Given the following data V(s) + 2 Cl₂(g) → VC14 (1) 1 VCl3(s) → VCl2 (s) + 2 Cl2(g) 2 VC13(s) → VCl₂ (s) + VC14 (1) calculate AH for the reaction: [-580.7 kJ] 3 V(s) + Cl2(g) → VCl3 (s) 2 AH= -569.4 kJ AH = +128.9 kJ ΔΗ = +140.2 kJ I
4. Use Hess's Law and the following data; CHale) + 202) CO2le) + 2H,0(g) AH = - 802 KJ + CO2(e) 2C0 + 2H2g) AH = + 247 KJ CH416) + H,0e) + 3H2(e) AH = + 206 KJ + To determine AH for reaction: CH4le) + % Ozle) » COe) + 2H2e)
On a sheet of paper, calculate AH for the following (fictional) reaction, using the given information (applying Hess Law). Upload a picture of your answer, showing all work. Solve for AH of: A2B (I) CD3 (g) + E2F (g) Given: Reaction AH (kJ) ½ G2B(g) + B2(g) - ½ A2B (I) -50.0 G2B(g) + 2B2(g) - CD 3(g) + E2F(1) -200.0 E2F(I) – E2F(g) E2F(g) 75.0 Attach File Browse My Computer
One of the reactions that destroys ozone in the upper atmosphere is NO(g) + 03 (g) ⇒ NO2 (g) + O₂(g) Substance and State ▲Gƒ° (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate AG (at 298 K) for this reaction. l\G° = Submit KJ
Answer the attached photo.
Another group performed the combustion of sucrose. Determine the AHcombustion (in kJ/mol) of sucrose given the following data obtained by the other group. Combustion Reaction: C12H22011 (s) + 1202 (9) → 12 CO2 (9) + 11H2O) Mole of sucrose: 0.0019 mol Ccal of the bomb calorimeter: 7876.2 J/°C AT:1.35 °C mass of burnt fuse wire: 0.0112 g qwire.surr: 5858 J/g
A student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.
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10) Given the following at 25°C, calculate AH, for HPO3(s) at 25°C P4010(s) + HNO3(1)– > HPO3(s) + N2O5(s) AH = -180.6 kJ AH, = -2984 kJ/mol for P4O10(s), -174.1 kJ/mol for HNO3(1), and - 43.1 kJ/mol for N2Os(s). a) -528.0 kJ/mol b) -1474 kJ/mol c) -943.7 kJ/mol d) +1474 kJ/mol e) -954.5 kJ/mol
how to solve this problem using the given at the top
Calculate H0rxn for each of the following using data from Appendix B. (a) 2 H2S(g) + 3 O2(g) 2 SO2(g) + 2 H2O(g) (b) C2H6(g) + O2(g) CO2(g) + H2O(g) [unbalanced](kJ)
D= Delta symbol Using Hess’s law (the indirect method) show how you can combine the following chemical reactions to determine the DHrxn for the following reaction. Zn (s) + 1/8 S8 (s) + 2 O2 (g) --> ZnSO4 (s) Goal: Determine DHrxn? Using the reactions below Zn (s) + 1/8 S8 (s) --> ZnS (s) DHrxn=A 2 ZnS (s) + 3 O2 (g) --> 2 ZnO (s) + 2 SO2 (g) DHrxn=B 2 SO2 (g) + O2 (g) --> 2 SO3 (g) DHrxn=C ZnSO4 --> ZnO (s) + SO3 (g) DHrxn=D