O Question 17 - Test 1 sem 2_20_2 XO https://ezto.mheducation.com/ext/map/index.html?_con3con&external_browser3D0&launchUrl=Saved20 21 1Enter your answer in the provided box.From the following heats of combustion,CH3OH(1) +,02(3) → CO2(g) + 2H,0(1)AH=-726.4 kJ/molrxnC(graphite)+ O2g)→ CO2(g)ΔΗ=-393.5 kJ/molrxnH;(g) + 0,(3) →→ H2O(!)AH= -285.8 kJ/molrxnCalculate the enthalpy of formation of methanol (CH,OH) from its elements:C(graphite) + 2H,(g) +0,() →→ CH3OH(1)kJ/mol< Prev17 of 20NeTarch

Answered: Image /qna-images/answer/d7513718-a0ba-447e-a16e-20c75f7fcf3d.jpg

Enter your answer in the provided box. From the following heats of combustion, CH3OH() +02(g) → CO2(g) + 2H,O(1) AH =-726.4 kJ/mol 2 rxn C(graphite) + O2g)→ CO2(g) AH =-393.5 kJ/mol rxn H2(3) + O2(g) H2O(1) AH =-285.8 kJ/mol rxn Calculate the enthalpy of formation of methanol (CH,OH) from its elements:

Enter your answer in the provided box. From the following heats of combustion, CH3OH() +02(g) → CO2(g) + 2H,O(1) AH =-726.4 kJ/mol 2 rxn C(graphite) + O2g)→ CO2(g) AH =-393.5 kJ/mol rxn H2(3) + O2(g) H2O(1) AH =-285.8 kJ/mol rxn Calculate the enthalpy of formation of methanol (CH,OH) from its elements:

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

The enthalpy (or heat) of combustion of acetone, (CH3)2CO, is - 1657.8 kJ. The reaction is (CH3)2CO (1) +4 0₂ (g) →3 CO₂(g) + 3 H₂O (g). Given the values of AH-393.5 kJ/mol for CO₂ (g) and AH-241.8 kJ/mol for H₂O(g), the calculated value of AH; for acetone O equals - 3563.7 kJ/mol O equals - 1022.5 kJ/mol O equals-248.1 kJ/mol O equals 1202.7 kJ/mol
18. From the following data, AH = -393.5 kJ/mol C(graphite) + O₂(g) → CO₂(g) 1 H₂ (g) + O₂(g) → H₂O(l) AH = -285.8 kJ/mol 2C₂H6 (g) +70₂(g) → 6H₂O(l) + 4CO₂(g) AH = -3119.06 kJ/mol calculate the enthalpy change for the reaction: 2C (graphite) (1) + 3H₂(g) → 2C₂H6 (g)
Calculate the enthalpy change for the following reaction, _C₂H4 (9) + using the following standard heats of formation: AH(C₂H4) = +52.5 kJ/mol; AH(CF4) =-933.0 kJ/mol; AH (HF) =-271.6 kJ/mol _F₂(g) → _CF4(g) + _HF(g)
Please help me, double and triple check your answers previous tutors got it wrong,
4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction: N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)
Calorimetry: Question #3 Octane, C3H18 , is a constituent of gasoline, and burns in the presence of oxygen to produce water and carbon dioxide: 2 C3H18 (1) + 25 O2(g) → 16 CO2(9) + 18 H2O1) ΔΗ kJ/2mol %3D rxn C3H18 (1) When a 1.00-gram sample of octane is burned in a bomb calorimeter the temperature of the water and the calorimeter rises from 25.00°C to 33.20°C. If the heat capacity, Cbomb cal, of the empty bomb calorimeter is 837 J/°C, and the mass of the water is 1.200 kg: a) Calculate the heat, q, transferred, during the combustion, to the calorimeter: 6.86 kJ (calorimter) + qbomb cal = Cbomb cal • AT b) Calculate the heat, q, transferred, during the combustion, to the water: 41.2 kJ (1.200 kg H20) + 9H20 = + mH20 • AT • SH2O c) Calculate the enthalpy change (AHº rxn = kJ/2mol) for this reaction (2 mol of C3H18 (1): [ Select ] kJ/2 mol C3H18 (1)
Given the enthalpies for the following reactions: 2 Fe (s) + 3/2 O₂(g) → Fe2O3 (s)Math output error AH₂ ΔΗ, CO (g) + 1/2 O₂ (g) → CO₂ (g) CO2 (g) ΔΗ = -248.7 kJ rxn rxn = 1,091.6 kJ Calculate the enthalpy change (AHrxn) for the following reaction: Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO₂ (g)
What is the enthalpy change when 2.00 mol of oxygen (O2) react? C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(l) ΔH = -5644 kJ
Given that enthalpy of formation of the several compounds: C(s)+O2(g)>CO2(g);AH=-393.5kJ S(s)+O2(g)→SO2(g);AH=-296.8kJ C(s)+2S(s)→CS2(1);AH=+87.9 kJ Determine the enthalpy of combustion reaction of carbon disulfide!
Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide. 2 C3H13 (2) + 25 02 (g) → 16 CO2(g) + 18 H2O(£) A,H° = -10,922 kJ/mol-rxn What is the enthalpy change if you burn 7.50 L of isooctane (d = 0.69 g/mL)? Enthalpy change |kJ =
The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d = 0.688 g/mL).
changé if 1.25 g of NO is completely converted into NO,? #36. Acetic acid, CH3CO2H, is made industrially by the reaction by the reaction of methanol and carbon monoxide. CH3OH(I) + CO2(g) CH;CO2H (1) H= -134,6 KJ/mol-rxn What is the enthalpy change for producing 1.00L of acetic acid ( d= 1.044g/mL) by this reaction? Op