2. Methylhydrazine (N₂H3CH3) is a common liquid propellant used in rocket fuels. Look for the standard molar enthalpies of formation of the reactants and products (you may use the uploaded files or search elsewhere for this). Calculate the AH° for the reaction. ° N2H3CH3 (l) + N2O4 ( ---> H₂O(g) + N2 (g) + CO2(g)

2. Methylhydrazine (N₂H3CH3) is a common liquid propellant used in rocket fuels. Look for the standard molar enthalpies of formation of the reactants and products (you may use the uploaded files or search elsewhere for this). Calculate the AH° for the reaction. ° N2H3CH3 (l) + N2O4 ( ---> H₂O(g) + N2 (g) + CO2(g)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 17E: Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or...

See similar textbooks

Similar questions

3. Use bond dissociation enthalpies to estimate the enthalpy change for the decomposition of hydrogen peroxide. 2 H2O2(g) → 2 H2O(g) + O2(g) +352 kJ/mol-rxn −206 kJ/mol-rxn +1037 kJ/mol-rxn −2204 kJ/mol-rxn
The table below contains some mean bond energy data: Bond C-C 348 H-H N=N Mean bond energy /kJ mol| 436 944 (i) Balance the equation below for the formation of one mole of ammonia, NH3, from its elements. N2 + H2 NH3 AH = -38 kJmol" (ii)Use the data in the table above to calculate the bond energy of N - H bond in NH3 in the reaction given in (1) above. Comment on why the value obtained is referred to as 'mean bond enthalpy (ii) Use the equation below and data from the table to calculate a value for the C=C bond energy in ethene. Bond H-H C-H C-C 348 Mean bond energy /kJ mol 436 418 нн нн С—С + Н Нэнс- с н AH = -136 kJ mol нн н Ethene Ethane
The term "bond energy" and "bond enthalpy" have often been used interchangeably to describe the strength of a bond. a) Calculate the average bond enthalpy of the O-H bond in water at 298 K and 1 bar, given the reaction: H₂O(g) →2H(g) + O(g), with AHƒ = 218.0, 249.2, and -241.8 kJ mol¹¹ for H(g), O(g), and H₂O(g) respectively. Give your answer in units of kJ/mol. b) How does your answer from (a) compare to the average bond energy (i.e. AU) of the O-H bond at 298 K and 1 bar: 461.0 kJ/mol?
P2D.9* Concerns over the harmful effects of chlorofluorocarbons on stratospheric ozone have motivated a search for new refrigerants. One such alternative is 1,1,1,2-tetrafluoroethane (refrigerant HFC-134a). A compendium of thermophysical properties of this substance has been published (R. Tillner- Roth and H.D. Baehr, J. Phys. Chem. Ref. Data 23, 657 (1994)) from which properties such as the Joule-Thomson coefficient u can be computed. (a) Compute u at 0.100 MPa and 300K from the following data (all referring to 300K): p/MPa 0.080 0.100 0.12 Specific enthalpy/(kJ kg"') 426.48 426.12 425.76 (The specific constant-pressure heat capacity is 0.7649kJ K' kg") (b) Com- pute u at 1.00 MPa and 350 K from the following data (all referring to 350 K): p/MPa 0.80 1.00 1.2 Specific enthalpy/(kJ kg") 461.93 459.12 456.15 (The specific constant-pressure heat capacity is 1.0392 kJ K¯' kg.)
Without referring to tables, predict which of the followinghas the higher enthalpy in each case: (a) 1 mol CO21s2 or1 mol CO21g2 at the same temperature, (b) 2 mol of hydrogenatoms or 1 mol of H2, (c) 1 mol H21g2 and 0.5 mol O21g2 at25 °C or 1 mol H2O1g2 at 25 °C, (d) 1 mol N21g2 at 100 °C or1 mol N21g2 at 300 °C.
6) Construct a graphical Born-Haber cycle for the formation of SrCl2(s). Explicitly label each transformation according to the chemical / physical change involved, and the thermochemical descriptor (i.e. AHatomization, AH lattice, IE, EA etc.). Relevant thermochemical data (in kJ/mol): For Sr: Enthalpy of sublimation: 164. IE₁: 549; IE2: 1064. For Cl: Electron affinity of Cl: -349. Enthalpy of dissociation for Cl₂: +243. Lattice energy of SrCl₂: -2150. Using these data, calculate the enthalpy of formation of SrCl₂.
Use average bond energies to compare the stabilities of allyl alcohol, CH2CHCH2OH, and acetone, (CH3)2CO, both of which have the same formula, C3H60. What is the difference in stabilities of the two compounds? Give the absolute value of the difference (positive value). i kJ eTextbook and Media Select all that apply to the stability of allyl alcohol and acetone. O Allyl alcohol is more stable due to difference in stabilities. O Acetone is more stable due to difference in stabilities. O Acetone is more stable than allyl alcohol. O Allyl alcohol is more stable than acetone.
If HO2 and HO4H were perfect gases, and vibrational motion of the molecules was ignored, what would the value of Cp be? Plot the heat capacities of each species over the range 200 K < T < 400 K. Do you think vibrational motion is significant in these molecules? (I have the equations for Temperature dependent entropies and heat capacities for both molecules plus their enthalpies of formation values at 298.15K. I am wondering how I would begin to solve this problem.)
unlv.instructure.com 7. Determine the change in enthalpy (AH) for the reaction:[1.5] CH3COCH3(1) +202(g) --> CH3COOH(I) + CO2(g) + H2O(g) Using the given information: CH3COCH3(1) +4 O2(g) --> 3 CO2(g) + 3 H20(I) AH = -1787.0 kJ H20(1) --> H2O(g) AH = -44.1 kJ CH3COOH(I) + 2 02(g) --> 2 CO2(g) + 2H2O(1) AH = -835.0 kJ 8.50.0 mL of 1.00 M HCI is mixed with 50.0 mL of 0.95 M KOH in a calorimeter with a caloriem constant (Kcall) of 17.3 J/°C. A change in temperature was observed from 26.0 °C to 32.6 °C. Wh
Indicate whether each statement is true or false. (a) Unlikeenthalpy, where we can only ever know changes in H, wecan know absolute values of S. (b) If you heat a gas suchas CO2, you will increase its degrees of translational, rotationaland vibrational motions. (c) CO2(g) and Ar(g) havenearly the same molar mass. At a given temperature, theywill have the same number of microstates.
eaching and lear X + Irn/takeAssignment/takeCovalentActivity.do?locator-assignment-... ☆ 9 Use the References to access important values if needed for this question. Given the standard enthalpy changes for the following two reactions: (1) N₂(g) +202(g) → 2NO2(g) (2) 2N₂O(g) → 2N₂(g) + O₂(g) What is the standard enthalpy change for the following reaction? (3) 2N₂O(g) + 302 (g) → 4NO2 (g) AH =? Standard enthalpy change = -297 An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Submit Answer 8 more group attempts remaining KJ Retry Entire Group AH = 66.4 kJ ΔΗ° = – 164.2 kJ Previous Next
P2C.4 From the following data, determine A,H° for diborane, B,H,(g), at 298 K: (1) B,H,(g) + 30,(g) → B,O,(s) +3 H,O(g) A̟H° =-1941kJ mol -> %3D (2) 2B(s) + 를0,(g) → B,O, (s) A̟H® =-2368 kJ mol (3) H,(g)+±O,(g) → H,O(g) A,H° =-241.8kJ mol %3D