From the following data: 1. Cigraphite) + O9) → CO9) kj AH = -393, 5- ran mol kj H9) +O2%0) H20) AH = -241,8- mol 2. ran 2C,H) + 7029) + 4CO9) +6H2O4) AH kj -3119, 6- 3. ran mol AHen kj = 44,0- mol 4 H2Ou) → H2O) Calculate the enthalpy change of standard reaction, AHrxn, (in kJ / mol) for the reaction of formation of one mole of ethane (C2H6(g) from the elements in their ground state
Q: (a) The ionization energy of potassium (K) is 4.34 eV and the electron affinity of chlorine (Cl) is…
A: a. Cohesive energy will be the negative of the Coulombic energy as given in Numerical, minus the…
Q: Kc=75.5 at 50°C for the re neaction Acgp + Beg) a ie What will be the a equiliorio ZAB g)…
A:
Q: Calculate the standard enthalpy of formation of WO3 (s) from W(s) and O2 (g) at 250C and 1 atm…
A: Hess's law:- " The enthalpy change of an overall process is the sum of the enthalpy change…
Q: Pala) +6 Cla(e)4 PCh() AH-7 enthaipy change for the formation of PC from the elements can be…
A: Given we know about the thermodynamic process of chemical reaction and find ∆rxH°
Q: Br. CH,C, (ooverte) os 1.0, 2. (CH,),S KMno, (hot.conc)
A: These reactions mainly involved highly reactive olefinic bond towards several potential reagents.
Q: E15C.5(a) Calculate the lattice enthalpy of CaO from the following data: AH/(kJ mol") Sublimation of…
A: Lattice enthalpy : The energy released when the ions combines, because of strong electrostatic…
Q: dy Q1. In a niaction to nuake nuanganise From manganess oxide, the Follocwing results whene…
A: Given in the reaction that : 1 mole of MnO2 gives 1mole of Mn and 1mole of O The reaction given is :…
Q: Use the molar bond enthalpy data in the table to estimate Bond kJ · mol-! Bond kJ · mol-! the value…
A: The enthalpy change of the reaction∆H∘rxn is equal to the difference in enthalpies of products and…
Q: Q.3. Find the equilibrium number of vacancies in 1m³ of Cu at 1000 °C. Vacancy formation energy per…
A: Introduction: In a solid state, vacancy arises due to absence of atom or molecules from a place that…
Q: X = X + 2, (9.30)
A: From the expression: χ=χi+λ where X: Susceptibility Xi: Contribution of the ions (core electrons) λ:…
Q: Q-6 Based on the experimental data below for Aluminum, determine (using Excel and by hand) the…
A:
Q: Element Atomic Atomic Radius E- configuration ( short Boiling Melting Standard 1st Point in…
A: The standard enthalpy of fusion is the heat (enthalpy) required to change the physical state from…
Q: The diameter of a rubidium atom is 4.95 A° . We will considertwo different ways of placing the atoms…
A:
Q: Carbon has an atomic radius of 77 pm and a first ionization energy of 1086 kJ/mole. 23. Based on…
A: Introduction : Ionisation energy : Ionization energy is simple terms can be described as a measure…
Q: Calculate the lattice enthalpy of CaO from the following data:…
A: For calculation of lattice energy we use Born Haber cycle. Lattice energy is amount of heat released…
Q: Calculate the boiling point of hydrogen peroxide round your answer to the nearest degree.
A: In thermodynamics entropy of vaporization is calculated by using below formula,
Q: Explain the difference in boiling points between PH3 and AsH3.
A: The boiling point of a liquid is its vapor pressure at a temperature equal to the gas pressure above…
Q: The diameter of a rubidium atom is 4.95 A° . We will considertwo different ways of placing the atoms…
A: (a) Given diameter = 4.95A0 = 4.95 × 10-8 cm
Q: the following reaction: N204 2NO2 Kc = 0.212 at 100°C Calculate AG° in J mol for the reaction. (R =…
A: Equilibrium reactions are chemical reactions in which the reactions are processed in both the…
Q: 6. Determine the DH° for CO(g) +1/2 O2 (g) CO2(g) rxn if C(graphite) +1/2 O2 (g) CO(g) DH° = -300…
A: According to Hess law of constant heat of summation, the total enthalpy change for a reaction is the…
Q: Using the data to the right, calculate the standard enthalpy change. Mt(s) + ½ O2(g) → MtO(s)…
A: The reaction given is
Q: McQuarrie Rock Gallogly presented by Macmillan Learning Use the molar bond enthalpy data in the…
A:
Q: Calculate the M.wt. of C,H14O2, CH;N,SO4, Na,CO, P2Os
A: The compound given are C7H14O2, C2H5N2SO4, Na2CO3, and P2O5.
Q: 8. A pure silicon cont ains 5 x 1028 atom per cubic meter and the ratio of brok en bonds are one…
A: The ratio of broken covalent bonds is given in the following step. As we know semiconductor metal…
Q: mol
A:
Q: A] Calculate AH° for the reaction C2H4g) + 3 Oze) 2 2002(g) + 2H½O(g) The average bond energies of…
A:
Q: 6.61 From these data, S(rhombic) + O2(g) SO-(g) AHn = -296.06 kJ/mol %3D S(monoclinic) + 0,(g) –→…
A:
Q: The AH rxn for which of the following reactions would have the same value in kJ/mol as the electron…
A:
Q: Using the following data, estimate AHF° (in kJ/mol) for potassium chloride: K(s) + ½ Cl2(g) →…
A: Given values: Lattice energy of KCl = -690 kJ/mol Ionization energy of K = 419 kJ/mol Electron…
Q: Given the bond enthalpy information below, calculate the Δ H of the following hypothetical reaction:…
A:
Q: Sketch diprem in dicating S-Po cess fath from 131 xe to 140 Ce . Specify tsbe of each behoce (ie,…
A: An element can have more than one isotope when there are nuclei that have different mass numbers but…
Q: Use the following data (in kJ/mol) to estimate AH for the reaction S (g) +e → s² (g) . Include an…
A:
Q: The ionization constant for HNO2 is 2.70 x 10-6 at 25 oC. Determine the standard free energy change…
A: The expression for standard free energy change is given below, R is the universal gas constant, T…
Q: 6- Draw Born - Haber Cycle and Calculate the lattice enthalpy for lithium fluoride, given the…
A: In this question, we want to determine the value of lattice energy ( U ) for LiF ( Lithium fluoride…
Q: 16. Calculate the normal melting point of l2 (s) in °C given the following data: AH° = 15.52 kJ/mol…
A:
Q: A. Determine the ASuniv of the following reactions at standard conditions: 1. 2CO(g) + 0,(g) 2co.(g)…
A: We know that entropy for the substance present in solid phase are considered as zero and entropy of…
Q: 15. Calculate the AH for the decomposition of one mole af nitroglycerin using the standard bond…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Discuss the factors affecting the sign of AG in the relationship AG= AH - TAS. Give examples for…
A: The relation ΔG = ΔH -TΔS is known as Gibbs Helmoltz equation We know that ΔG is always negative for…
Q: value of Ksp be for calcium fluoride?
A:
Q: Power Index = 178% Heat of explosion (Qv) = 6666kJ/kg Gaseous products detected: CO2, H2O, and N2…
A: Given : Power Index = 178% Heat of explosion (Qv) = 6666kJ/kg
Q: Using the values provided in the table below, calculate ΔS for the following reaction: O2(g) +…
A: The entropy of a chemical reaction can be calculated by taking the difference between the entropy of…
Q: Please provide an explanation for the relatively high boiling points of H20, HF, and NH3 in…
A: Boiling point of any compound depends on the intermolecular forces of attraction. More strongly the…
Q: Determine ASm for H2(g) + I,(g) = 2HI(g) given the following informatic Substance S° (J/mol · K)…
A: Introduction: We have to calculate entropy. Given:
Q: Consider a hypothetical ionic compound AB (comprised of A+ and B- ions). Given the following…
A:
Q: Using the values provided in the table below, calculate AS for the following reaction: 2SO3(g) O2(g)…
A: Given Reaction2 SO3(g) → O2(g) + 2SO2(g) Species S° (J/mol.K) SO2(g) 248 SO3(g) 114…
Q: 8. A pure silicon cont ains 5 x 1028 at om per cubic met er and the ratio of brok en bonds ar one…
A:
Q: Given Zn(s) and AL(s), what observations would you make when combining AL(s) with ZnSO4(aq), and…
A: when combining Al(s) with ZnSO4(aq) then the reaction will take place because Aluminium is more…
Q: Using the following data, estimate AHf° for potassium chloride: K(s) + ½ Cl2(g) → KC(s). Lattice…
A:
Q: Find the ao ve al values of hypochloros deid in a dolu tion ith. a of 7.0.(kaHOCI 3x10-8 for Hacil…
A:
Must answer all and properly else downvote
Step by step
Solved in 2 steps
- ) Given the following data on Phosphorus and its allotropeso ∆Hf kJ mol-1 ∆Gfo kJmol-1 So J mol-1 K-1 White phosphorus, P(s, white) 0 0 0 Gaseous Phosphorus, P(g) 315 278 163 Gaseous Phosphorus, P4(g) 59 24 280 b) For the transformation P(g) -> ¼ P4(g), is work done by the system or on the system? How much work is involved? Explainwith solutions. c) Calculate the ∆E in kJ for the process P(g) ¼ P4(g) in (b). d) Calculate the sublimation temperature for white Phosphorus (in oC) assuming constant values of enthalpy and entropyover the temperature range involved.1. Use the following reactions to determine the Delta Hrxn for P4O10(s) + 6H2O(l) 4H3PO4(l) 4P(s) + 5O2(g)---> P4O10(s). Delta H = -2984kJ 2H2(g) + O2(g)---> 2H2O(l) Delta H = -570kJ 2P(s) + 4O2(g) + 3H2(g)---> 2H3PO4(l). Delta H = -2534kJ B. Is the reaction exothermic or endothermic? C. Given Sof P4O10(s) = 228.9 J mol-1 K-1; Sof H2O(l) = 69.9 J mol-1 K-1; Sof H3PO4(l) = 241.98 J mol-1 K-1 calculate the DGrxn at 28.0oC. D. Is this reaction spontaneous or nonspontaneous?P2C.6 For the reaction Cr(C6H6)2(s) → Cr(s) + 2C6H6(g), ΔrU⦵(583K) = +8.0 kJmol−1. Find the corresponding reaction enthalpy and estimate thestandard enthalpy of formation of Cr(C6H6)2(s) at 583K.
- Use the table below to answer the questions that follow.Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C)Substance ΔH°f (kJ/mol) ΔG°f (kJ/mol) S (J/K-mol) Substance S° (J/K-mol) CO2 (g) 213.6 C2H2 (g) 200.8 O2 (g) 205.0 H2O (l) 69.91 Calculate the value of ΔS° (J/K ∙ mol ) for the catalytic hydrogenation of acetylene to ethane,C2H2 (g) + 2H2 (g) → C2H6 (g)#4 Find ΔGo for the following reaction, at 25°C, using ΔHof and So values. NH4Cl(s)→NH3(g) + HCl(g) =____kJ Standard Thermodynamic Values at 298 K Substance or Ion ΔHof(kJ/mol) So(J/mol K) HCl(g) −92.3 186.79 HCl(aq) −167.46 55.06 NH3(g) −45.9 193 NH3(aq) −80.83 110 NH4Cl(s) −314.4 94.6For the reaction C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g), ΔrU⦵ = −1373 kJ mol−1 at 298 K. Calculate ΔrH⦵.
- Estimate the boiling point of ethanol given the following thermodynamic parameters. C2H5OH(l) C2H5OH(g) ΔfH° (kJ/mol) –277.0 –235.3 S° (J/K-mol) 160.7 282.7 ΔfG° (kJ/mol) –174.7 –168.5Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K. 2 H(g) ⇌ H"(g) or equivalently H(g) + H(g) ⇌ H2(g) Δf?° (kJ mol-1) ?° (kJ K-1 mol-1) H(g) 218.0 0.115 H2(g) 0 0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.Using the data below, the ∆S⁰ is -326.3 J/K in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K. Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 TRUE OR FALSE
- Determine ∆G° for the phase change CO₂(g) → CO₂(aq) at 25°C. delta H = -19.4 kJ/mol delta S= 92.3 J/mol*k Temp=25CA sample of K(s) of mass 3.226 gg undergoes combustion in a constant volume calorimeter at 298.15 K. The calorimeter constant is 1849 J⋅K−Mol-, and the measured temperature rise in the inner water bath containing 1538 gg of water is 1.776 K. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1CP,m(H2O,l)=75.3J⋅mol−1⋅K−1. 1) Calculate ΔU���f for K2O 2) Calculate ΔH∘f for K2OWhen the work done on a system (+delta G) to bring it into an ordered state (negative delta S), which of the following is true?