Use the following data to calculate the A H for the reactionCH4 (g) C (9) + 4H (g) given the following data:C (gr) + 2H2(g)-> CH4(g) delta H = - 74,7 kJ/molH2 (g) - 2H (g) delta H = +436 kJ / molC (gr) --> C (g) delta H = +716.7 kJ/molO +1663.4 kJ/ molO -206 kJ / molO-1078 kJ / molO- 1663.4 kJ/ molO +1078 kJ/ mol

Given data Reaction (1) C(gr)+2H2(g)→CH4(g) , ∆H1 =-74.7 KJ/moleReaction (2)…

Answered: Use the following data to calculate the…

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

Calculate the AH°rxn for the combustion of methane using the given AH°r. CH4 (g) + 202 (g) 2H20 (1) + CO2{g) AH°t, methane(g) = -74.60 kJ/mol AH°f, water(l) = -285.8 kJ/mol AH°t, carbon dioxide(g) = -393.5 kJ/mol 890.5 kJ/mol -890.5 kJ/mol -1.04 x 103 kJ/mol
Use the information provided to determine AH°rxn for the following reaction: -> CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) AH°rxn = ? AHof (kJ/mol) CH4(g) -75 CCl4(g) -96 HCl(g) -92 O A.-71 kJ O B.-389 kJ OC. +79 kJ O D. +113 kJ O E.-113 kJ
Using the provided table, determine the enthalpy for the reaction C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AH¡ (kJ/mol) C3H® (g) -108.4 O2 (g) CO2 (g) -393.5 H2O (g) -241.8
Another group performed the combustion of sucrose. Determine the ΔHcombustion (in kJ/mol) of sucrose given the following data obtained by the other group. Combustion Reaction: C12H22O11(s)+12CO2(g)+11H2O(l) Mole of sucrose: 0.002 mol Ccal of the bomb calorimeter: 7943.1 J/ºC increment T: 1.36 ºC mass of burnt fuse wire: 0.0108 g qwire,surr: 5858 J/g Express your answer in 2 decimal places. Round your answer to 2 decimal places.
Calculate ΔH orxnfor the following: CH4(g) + Cl2(g) → CCl4(l) + HCl(g)[unbalanced]ΔH o/f[CH4(g)] = −74.87 kJ/molΔH o/f[CCl4(g)] = −96.0 kJ/molΔH o/f[CCl4(l)] = −139 kJ/molΔH o/f[HCl(g)] = −92.31 kJ/molΔH o/f[HCl(aq)] = −167.46 kJ/molΔH o/f[Cl(g)] = 121.0 kJ/mol
Using the provided table, determine the molar enthalpy (in kJ/mol) for the reaction C₃H₈ (g) + 5 O₂ (g) → 3 CO₂ (g) + 4 H₂O (g) Substance ∆Hf° (kJ/mol) C₃H₈ (g) -108.4 O₂ (g) 0 CO₂ (g) -393.5 H₂O (g) -241.8
Hh.190.
1) From the following data, C(graphite) + O2(g) à CO2(g) = -393.5 kJ/mol H2(g) + 1/2O2(g) = H2O(l) delta H = -285.8 kJ/mol 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(l) delta H = -3119.6 kJ/mol calculate the enthalpy change for the reaction 2C(graphite) + 3H2(g) =C2H6(g) a) –2417.2 kJ b) –84.6 kJ c) 2417.2 kJ d) –3204.2 kJ
Given the following information: Pb(s) + PbO2(s) + 2H2SO4(l) ---> 2PbSO4(s) + 2H2O (l) DHrxn = 509.2 KJ/mol SO3 (g) + H2O (l) ---> H2SO4 (l) DHoRxn = -130.3KJ/mol Determine DHoRxn for: Pb (s) + PbO2(s) + 2SO3 (g) ----> 2PbSO4 (s)
Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) Reaction 2: Reaction 3: - 20F 2(g) ->> O2(g) + 2 F2 (g) AH = -49.4 kJ 2HCl(g) AH = -184.6 kJ N₂(g) +202 (8) -> Use Reaction 2. Answer: How much energy (in kJ) is released when 71.0 g of oxygen difluoride decomposes? Enter a positive number. Round to the nearest hundredth. 2NO2(g) AH = +66.4 kJ KJ
22c

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS