Construct a Born-Haber cycle for Ga (s) + Cl2(g) → GaCl3(s) and calculate the enthalpy of formation for GaCl3 using the following data. Remember what I said about constructing a cycle; you need to do this properly. AHf = ? AH3rd= 2965 kJ AHsub = 277 kJ AH1st IE = 579 kJ AHBD = 244 kJ AH2nd IE = 1979 kJ %3D AHEA = -364 kJ LE = -3091 kJ

Construct a Born-Haber cycle for Ga (s) + Cl2(g) → GaCl3(s) and calculate the enthalpy of formation for GaCl3 using the following data. Remember what I said about constructing a cycle; you need to do this properly. AHf = ? AH3rd= 2965 kJ AHsub = 277 kJ AH1st IE = 579 kJ AHBD = 244 kJ AH2nd IE = 1979 kJ %3D AHEA = -364 kJ LE = -3091 kJ

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

Calculate how much energy would be needed for 64.8 g titanium at 19.4 oC to reach 582 degrees Celcius.
1. Given the following information, calculate the lattice energy for LiI(s). Show all work and construct a diagram(cycle) that shows each step in the process of forming LiI(s) from gaseous ions.
The combustion of propane gas (C3H8; molar mass = 44.09 g/mol) occurs according to the following equation: C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g) Given the following standard molar enthalpy of formation (DHof), how much energy in kilojoules is produced when 1.00 g of propane is completely combusted? DHof[C3H8] = -103.8 kJ/mol; DHof[CO2] = -393.5 kJ/mol, and DHof[H2O(g)] = -241.8 kJ/mol (A) 2043.9 kJ (B) 531.5 kJ (C) 12.1 kJ (D) 46.4 kJ
After reading the information from a answer B
A scientist measures the standard enthalpy change for this reaction to be 296.0 kJ/mol: H₂S(g) + 2 H₂O(l) 3H₂(g) + SO₂(g) Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of H₂S(g) is kJ/mol. Submit Answer Retry Entire Group 1 more group attempt remaining
How do I calculate Δf H of MgCl(s) given the following data? Enthalpy of sublimation for Mg(s) = + 146 kJ/mol enthalpy of dissociation of Cl2 (g)= +244 kJ/mol electron affinity of Cl- = -349 kJ/mol first ionization energy of magnesium Mg (g) = 738 kJ/mol lattice energy of MgCl(s) = -676 kJ/mol.
A) 425.66J/2.0360 g. Convert to kj/mol. Show the work. Molar mass = 39.99 NaOH B) 425.32J/ 1.9532g. Convert to kj/mol. Molar mass = 80.043 Na4NO3
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
Given the reactions and the heats of reaction associated with them, use Hess' Law to calculate the heat of formation of SO2(g). S(s) + 3/2 O2(g) → SO3(g) ΔH = -395 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH = -198 kJ
A model for the compound 2,2- dimethylbutane is shown. Write a balanced chemical equation that shows the formation of 2,2-dimethylbutane from the elements carbon (C) and hydrogen). (Use the smallest integer coefficients possible and do not include states.) A model for the compound 2,2-dimethylbutane is shown Write a balanced chemical equation that shows the formation of 2,2-dimethylbutane from the elements carbon (C) and hydrogen (H₂) (Use the smallest integer coefficients possible ond do not include states.)
How much energy would need to be applied to 654 g platinum to raise it from 25.0 degrees C to 486 degrees C?