I Review | Constants | Periodic TableHess's law states that "the heat released or absorbed in achemical process is the same whether the process takes placein one or in several steps." It is important to recall the followingrules:Part A1. When two reactions are added, their enthalpyvalues are added.2. When a reaction is reversed, the sign of itsenthalpy value changes.3. When the coefficients of a reaction are multipliedby a factor, the enthalpy value is multiplied by thatCalculate the enthalpy of the reaction2NO(g) + O2(g)-2NO, (g)given the following reactions and enthalpies of formation:same factor.1. N2(g) + O2(g)→NO2(g), AH = 33.2 kJ2. N2 (g) + 02(g)→NO(g), AH = 90.2 kJExpress your answer with the appropriate units.• View Available Hint(s)AH =ValueUnitsSubmit II Review | Constants | Periodic TableHess's law states that "the heat released or absorbed in achemical process is the same whether the process takes placein one or in several steps." It is important to recall the followingrules:AH° =ValueUnits1. When two reactions are added, their enthalpyvalues are added.2. When a reaction is reversed, the sign of itsenthalpy value changes.3. When the coefficients of a reaction are multipliedby a factor, the enthalpy valueSubmitmultiplied by that• Part Bsame factor.Calculate the enthalpy of the reaction4B(s) + 302 (g)→2B2O3 (s)given the following pertinent information:1. B2O3 (s) + 3H20(g)-302(g) + B2H6 (g),2. 2B(s) + 3H2 (g)→B2 H6 (g),3. H2 (g) + +02(g)→H20(1),4. H20(1)→H20(g),AH = +2035 kJAH = +36 kJAH = -285 kJAH = +44 kJExpress your answer with the appropriate units.> View Available Hint(s)AH° =ValueUnitsSubmit

Answered: Image /qna-images/answer/370eba2f-a7f8-46c9-beb9-8d94a4e60423.jpg

Part A Calkulate the enthalpy of the reaction 2NO(g) + Oz(x)→2NO;(g) given the following reactions and enthalpies of formation: 1. N2(g) + O2(8)→NO2(g), AH¡ = 33.2 kJ 2. +N2(g) + +O2(8)→NO(g), AĦ = 90.2 kJ Express your answer with the appropriate units. • View Available Hint(s) HA

Part A Calkulate the enthalpy of the reaction 2NO(g) + Oz(x)→2NO;(g) given the following reactions and enthalpies of formation: 1. N2(g) + O2(8)→NO2(g), AH¡ = 33.2 kJ 2. +N2(g) + +O2(8)→NO(g), AĦ = 90.2 kJ Express your answer with the appropriate units. • View Available Hint(s) HA

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

Which of the following reactions corresponds to the standard enthalpy of formation of methane CH4? A: C(s, gr) + 2H2(g) —> CH4(g) B; CH4(g) —> C(s, gr) + 2H2(g) C: C(s,gr) + 4H (g) —> CH4 D:CH4–> C(s,gr) + 4H(g) Choose one. Thanks!
4 CH3NH2 (g) + 2 H2O (l) ➝ CO2 (g) + 3 CH4 (g) + 4 NH3 (g) ΔHº = –138.96 kJ• Calculate the overall change in enthalpy when 30.00 grams of CH3NH2 (g) reacts with excess H2O (l). [Be sure to include the correct sign.]
Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2 H40, by the reaction C2 H4O(g) + H,0(1) HOCH, CH,OH(!) Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C, HO(g) + 502(9) → 4CO2 (9) + 4H,0(1) AH =-2612.2 kJ HOCH, CH, OH(1) + O2 (9) → 2002 (9) + 3H,0(1) AH=-1189.8 kJ Enthalpy change = kJ %3D
Given the two thermochemical equations below, find the enthalpy change for the reaction: N2H4 (l) + H2 (g) → 2 NH3 (g) delta H = ? Given: N2O4 (g) + 3 H2 (g) → 2 NH3 (g) + 2 O2 (g) delta H = – 100.96 kJ N2O4 (g) + 2 H2 (g) → N2H4 (l) + 2 O2 (g) delta H = + 41.47 kJ Select one: a. – 142.43 kJ b. – 59.49 kJ c. + 41.47 kJ d. + 59.49 kJ e. + 142.43 kJ f. none of these g. – 100.96 kJ
For which one of the following is the enthalpy of the reaction the same as the enthalpy of formation? A) 2 H (g) + Se (s) → H:Se (g) B) KOH (s) → K*(aq) + OH- (aq) C) 2 Fe (s) + 3 Cl2 (g) → 2 FeCl3 (s) D) Ni (s) + ½ O2 (g)- NiO (s)
and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8
From the following data, C (graphite) + O₂(g) → CO₂(g) H₂(g) + —⁄- 02₂(g) → H₂O (1) CH₂(g) + 20₂(g) → CO₂(g) + 2H₂O (1) kJ ×10 Calculate the enthalpy change for the reaction below: C(graphite) + 2H₂(g) CH4 (g) Be sure your answer has the correct number of significant digits. X → ΔΗ° S rxn ΔΗ° = -285.8 rxn = -393.5 ΔΗ° = -890.4 rxn kJ mol kJ mol kJ mol
Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84
The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04
In the laboratory, a student dilutes 17.8 mL of a 9.80 M hydrobromic acid solution to a total volume of 125.0 mL. What is the concentration of the diluted solution? Concentration = 0.78 M
Calculate the enthalpy of formation of 1 mole SO₂(g) from the standard enthalpy changes of the following reactions: 2SO3(g)2SO₂(g) + O₂(g) 2S (s) +30₂(g) → 2SO3(g) →→ SO₂(g) S(s) + O₂(g) kJ ΔΗ AH rxn 1=+196 kJ rxn 2 = -790 kJ AHO rxn 3 = ? k
Please answer the question in the image with details.