LIOh for each substance in Appendix C: (a) H2O2(g), (b) CaCO3(s), and then 1OUR up new tion any, (c) РОСІ: (1), (а) СH;ОН(). 6.71 The following is known as the thermite reaction: 2 Al(s) + Fe,O3(s) → Al2O3(s) + 2 Fe(s) This highly exothermic reaction is used for welding massive units, such as propellers for large ships. Using standard en- thalpies of formation in Appendix C, calculate AH° for this e reaction. cou

LIOh for each substance in Appendix C: (a) H2O2(g), (b) CaCO3(s), and then 1OUR up new tion any, (c) РОСІ: (1), (а) СH;ОН(). 6.71 The following is known as the thermite reaction: 2 Al(s) + Fe,O3(s) → Al2O3(s) + 2 Fe(s) This highly exothermic reaction is used for welding massive units, such as propellers for large ships. Using standard en- thalpies of formation in Appendix C, calculate AH° for this e reaction. cou

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 5.36QE: When lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO:...

See similar textbooks

Similar questions

The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
When lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO: N2(g)+O2(g)2NO(g)H=+181.8kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = +181.8 kJ? (c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess O2(g)?
Why is it important to give the states of the reactants and products when giving an equation for H?
If an equation for a reaction is doubled and then reversed, how is the value of H changed?
A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.
When one mole of ethylene gas, C2H4, reacts with fluorine gas, hydrogen fluoride and carbon tetrafluoride gases are formed and 2496.7 kJ of heat are given off. What is Hf for CF4(g)?
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: Na(g) + 3H,(g) – 2NH;(g) In the second step, ammonia and oxygen react to form nitric acid (HNO) and water: NH,(g) + 20,(g) HNO-(g) + H,0(g) Suppose the yield of the first step is 70.% and the yield of the second step is 61.%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.
(Q77) The standard Gibbs free energy (AG°rxn) for the formation of sulfur trioxide from sulfur dioxide and oxygen gas is -72.3 kJ/mol. The balanced chemical equation is SO2 (g) + ½ O2 (g) --> SO3 (g). What will be the Gibbs Free energy of the reaction (in kJ/mol) if it takes place at a low temperature of -13.7 and the concentrations of three gases are: SO2 = 0.112 M %3D O2 = 0.110 M SO3 = 1.74 M
process for yithenis of benzoin : (b) The followng eaction is a important process for yuthenis of benzoin O OH -CHO Find out the non Green' factor in this reaction. Suggest a Green alternative for this reaction, stating the benefits of the new process. Provide a Green alternative for the (6) following reaction and 'atom efficiency' of both the processes : compare the COOH COOH NaNOg H280, NO
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by réforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2(9)+3 H,(g)→2NH;(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH;(g)+2O,(9)→HNO,(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced. Explanation Check O2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility 2:53 PM 4/8/2022 DELL PrtScr Insert Delete PgUp PgDn F7 F8 F9 F10 F11 F12 Esc F1 F2 F3 F4 F5 F6 Fn Num 24 & ( ) Lock Backspace 1 2 6. 7 + II * 00 %#3
The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application todaY, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H, SO,() – SO;(9) + H,O() AH-+113. kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) – PbO,(s) - 2 S0, (g) → 2 PbSO,(s) AH= -775. J Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ.
Write the balanced NET ionic equation for the reaction when aqueous BaCl2 and aqueous (NH4)2SO, are mixed in solution to form aqueous NH,CI and solid BaSO4. O4- 3. 2. 2+ 3+ 4+ 1 2. 3 4 6. 7 8. 9. 4 7 8. 69 1. (s) (1) (g) (aq) Ba CI Reset • x H2O Delete SI 5.

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

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: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

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

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: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry