Please explain how to get answers 11/1 pointUse the accompanying AHOf values for the reaction: 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g). Select all correct answers below.SpeciesNH3 (g)02 (g)NO (g)H2O (g)AH°(kJ/mol)-46090-242>ΔΗ= -908 kJAS surr=AS° 03.05 kJ K-1The reaction is not spontaneous at 298 K

Given reaction: 4NH3 (g) + 5O2 (g) ---> 4NO (g) + 6H2O (g) The enthalpy change for a…

Answered: 1 1/1 point Use the accompanying AHOf…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.84QE

See similar textbooks

Similar questions

1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change to decompose 1.00 mol of HgO(s) to O2(g) and Hg(l)? 3633 kJ −90.8 kJ 90.8 kJ 363.3 kJ
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50 M NaOH in a StyrofoamTM cup calorimeter. Both solutions were initially at 20.0 C, but when the two were mixed, the temperature rose to 23.2 C (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 ml of 0.50 M NaOH. WIII the AT observed be greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCI and 100.0 ml. of 1.00 M NaOH. Will the T observed be greater than, less than, or equal to that in the first experiment, and why?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
ap chemistry
Name: m NetID: 17. Given the following set of reaction data, H2 (8) + 02(8) –H,O(1) 2B(s) +3H2(g) → B,H6(g) 2B(s) + O2(g) – B,O3(s) AH = -285.83 kJ mol-1 AH= 36.4 kJ mol- AH = –1273.5 kJ mol¬1 wilc pd mol determine the heat of reaction (in kJ mol¯l) for the following reaction. B2H, (g) + 302(8) B2O3(s) + 3H2O(1) lo sb 1ooleps laoin bss jo bra usido AH = ? kJ mol-1 s 26 air jes o s be noi A: -2167 s heet t
Please help
* 42) Given the following reactions N2 (g) + Del AH = +180.7 kJ O2 (g) → 2NO (g) 001.0 to Jm 0.25 nixim yd sbsa notulossa Im AH = -113.1 kJ 2NO (g) + O2 (g) → 2NO2 (g) ->> 0080.0 (C the enthalpy of reaction for acr (af DIMM 900 02.00.0 (A rlos M aansugs as to (M) noitsusid ladom s 4NO (g) 2NO2 (g) + N2 (g) 1008.0 000 (8 is _ kJ. TA) 67.6 B)-293.8 gdong C) 293.8 mo D) 45.5 to hustom E)-45.5 SESIA diation has the greatest
12
Q\4: The chemical change that describing methane {#C#} production is AH° -74.9 KJ. mole-1 C (s) + 2H₂ (g) → CH4 (9) Calculate the energy of (C-H) bond according to the following data. Atom C H (15 degree) AH for one mole of gas atoms (KJ.mol-¹) 715 218
Calculate AH° and AE° for the following reactions at 25 °C. Use standard enthalpies of formation from the table below. Round your answers to four significant digits. Substance AH; (kJ mol-1) Substance AH: (kJ mol-1) Co,(g) -393.5 226.75 Ni(g) C,H,(g) (CH3),CO(/) H,O(g) HC(g) NH,(g) -46.19 -248.1 NH.CIG) N,O(g) O(g) -315.4 -241.8 81.57 -92.30 (a) 2C2H2(g) + 502(g)4CO2(g) + 2H20(g) AH° = i kJ AF° = kJ eTextbook and Media (b) C2H2(g) + 5N20(g) → 2CO2(g) + H2O(g) + 5N2(3) AH° = i kJ AE° = i kJ
11? Please also address what ion of germanium is most likely to form!

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

1 1/1 point Use the accompanying AHOf values for the reaction: 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g). Select all correct answers below. Species NH3 (g) 02 (g) NO (g) H2O (g) AH°(kJ/mol) -46 0 90 -242 > ΔΗ = -908 kJ AS surr = AS° 0 3.05 kJ K-1 The reaction is not spontaneous at 298 K