Consider the table. Metal Tm (K) AĦfus (kJ/mol) |Tp (K) AH vap (kJ/mol) Li 454 2.99 1615 134.7 Na 371 2.60 1156 89.6 K 336 2.33 1033 77.1 Rb 312 2.34 956 69 Cs 302 2.10 942 66 Using the data, calculate ASfus and ASvap for K. AS vap J 77.51 K-mol Incorrect J AS fus = 7.0080 %3D K-mol

Consider the table. Metal Tm (K) AĦfus (kJ/mol) |Tp (K) AH vap (kJ/mol) Li 454 2.99 1615 134.7 Na 371 2.60 1156 89.6 K 336 2.33 1033 77.1 Rb 312 2.34 956 69 Cs 302 2.10 942 66 Using the data, calculate ASfus and ASvap for K. AS vap J 77.51 K-mol Incorrect J AS fus = 7.0080 %3D K-mol

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

Consider the following data: AH° (kJ/mol) 2CIF + O₂ + Cl₂O + F₂0 2CIF3+ 20₂(g) → Cl₂O + 3F₂0 167.4 341.2 2F2+ O2 → 2F₂0 Use Hess' law to find the change in enthalpy, AH, at 25°C for the following equation: CIF3 → CIF + F2 -43.4
The stratospheric ozone (O3) layer helps to protect usfrom harmful ultraviolet radiation. It does so by absorbingultraviolet light and falling apart into an O2 molecule and anoxygen atom, a process known as photodissociation.O3(g)----->O2(g) + O(g) Use the data in Appendix C to calculate the enthalpy changefor this reaction. What is the maximum wavelength a photoncan have if it is to possess sufficient energy to cause thisdissociation? In what portion of the spectrum does thiswavelength occur?
Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) → H,0(g) AH1 = -241.8 kJ 2) X(s) + 2 Cl,(g) → XCl,(s) AH2 = +475.9 kJ 3) H,(g) + CL,(g) HCl(g) АНз 3 —92.3 kJ → 4) X(s) + O,(g) –→ XO,(s) AH4 = -748.7 kJ 5) Н, О(2) — н,00) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2H,О() — ХО,(8) + 4 HCI(g)
How much energy is required to break the bonds in the molecule of NO, BCl3, and NO2? and How do I find the ΔH of the molecule from the elements in their standard states?
(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.
Suppose that the reaction of 1.38 grams of X (MW = 56.76) consumes 6.82 x 104 joules of heat. What is the molar enthalpy of the reaction in kJ/mol? Report your answer to three decimal places (ignore significant figures).
THERMOCHEMISTRY 237 23 3. A student wishes to determine the enthalpy of the reaction of hydrogen gas with chlorine gas by the reaction represented below. A high-pressure bomb calorimeter is used for this experiment. A 500.-mL high-pressure cell is filled with an equimolar mixture of H,(g) and CL,(g) to a total pressure of 10.00 atm and 293.50 K. H,(g) + CL(g) → 2 HCI(g) (a) If the reaction goes to completion, how many moles of HClI(g) can be produced? (b) The high-pressure sealed cell was placed in the bomb calorimeter and the mixture was ignited with an internal spark. The temperature of the calorimeter rose from 293.50 K to 298.83 K. If the previously-measured heat capacity of the whole calorimeter was C 3.60 kJ/K, calculate the heat transferred to the calorimeter by the reaction. (c) Calculate the experimental enthalpy of reaction in kJ/moln
Cl2 (g) + H2 (g) → 2 HCl (g) ΔH0rxn = ‒184.6 kJ 8. What is ΔH0rxn when 4.50 mol HCl (g) forms? (Slides 17 – 18: Stoichiometry of Thermochem. Eq.) Group of answer choices A.‒831 kJ B.‒415 kJ C.‒207 kJ D.831 kJ E.415 kJ
Given the following thermochemical equations: 4 FeS2(s) + 11 O2(g) 2 H2S(g) + 3 O2(g) → 2 Fe2O3(s) + 8SO2(g) → 2 H₂O(1) +2 SO2(g) →2 Fe2O3(s) 4 FeO(s) + O2(g) →2 FeO(s) 2 Fe(s) + O2(g) H2(g) +S(s) 2 H2(g) + O2(g) → H₂S(g) → 2 H₂O(1) Compute the AH for FeS2(s) in kJ/mol. A)-1233.9 kJ/mol B) -2893.9 kJ/mol C) -24.3 kJ/mol D) -183.5 kJ/mol E) -70.0 kJ/mol O A OB Oc OD OE (kJ/mol) ΔH° = -3307.9 - 1125.2 -578.2 -544 - 20.2 -571.7
Fluorine (F2), the most electronegative element reacts with water in a different way compared to other halogens do. With excess water, fluorine reacts with water to produce hydrofluoric acid and oxygen gas in the following reaction: 2F2(g) + 2H2O() →4HF (1) + O2(g) Calculate AHrxn for the process above from the following information: AH= +571.6 kJ (a) AH= +542.0 kJ (b) 2H₂O(1)→ 2H2(g) + O2(g) 2HF (g) → H2(g) + F2(g) Which equation(s) will you flip? O a. Only equation (b) O b. Only equation (a) O c. Both equations will be flipped. O d. No equations will be flipped.
Determine AH for the following reaction, N₂(g) + 3 H₂(g) → 2 NH3(g) given the thermochemical equations below. N₂(g) + O₂(g) → 2 NO(g) 4 NH3(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) 2 H₂(g) + O₂(g) → 2 H₂O(g) A. -1209.0 kj B.-1189.0 kJ OO OC. 150.3 k OD.-241.8 kJ E. -91.5 kJ Reset Selection o Ei C 6 AH = +180.8 kJ AH = -906.2 kJ ΔΗ = -483.6 k S IA
3. Write a balanced chemical reaction for the synthesis of methane (CH4) and liquid water from hydrogen and acetic acid (CH3COOH) and calculate the standard enthalpy of the reaction by using the appropriate enthalpies of formation on page 308 or Appendix 4 in the textbook.