Given the following information, construct a Born-Haber cycle to calculate the lattice energy of CaC2(s): Net...
Given the following information, construct a Born-Haber cycle to
calculate the lattice energy of CaC2(s):
Net energy change for the formation of CaC2(s)=−60kJ/mol
Heat of sublimation for Ca(s)=+178kJ/mol
Ei1 for Ca(g)=+590kJ/mol
Ei2 for Ca(g)=+1145kJ/mol
Heat of sublimation for C(s)=+717kJ/mol
Bond dissociation energy for C2(g)=+614kJ/mol
Eea1 for C2(g)=−315kJ/mol
Eea2 for C2(g)=+410kJ/mol
Express your answer using four sig figs
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Given the following information, construct a Born-Haber cycle to
calculate the lattice energy of CaC2(s):
Net...
Construct a Born-Haber cycle and calculate the lattice energy of CaC2 (s). Note that this solid...
Construct a Born-Haber cycle and calculate the lattice energy of CaC2 (s). Note that this solid contains the diatomic ion C22–.Useful Information:?H°f (CaC2(s)) ?Hsub (Ca (s)) ?Hsub (C (s)) Bond dissociation energy of C2 (g) = +614 kJ/molFirst ionization energy of Ca (g) = +590 kJ/mol Second ionization energy of Ca (g) = +1143 kJ/mol First electron affinity of C2 (g) = –315 kJ/mol Second electronaffinity of C2 (g) = +410 kJ/mol= –60 kJ/mol = +178 kJ/mol = +717 kJ/mol
7. Use the Born Haber cycle and the given information to determine the net energy change...
7. Use the Born Haber cycle and the given information to determine the net energy change (in kJ/mol) that takes place in the formation of KF(s) from the elements: Ks) + F2@KFS) Heat of sublimation of K = 89.2 kJ/mol Bond dissociation energy for F2 = 158 kJ/mol Lattice Energy of KF = 821 kJ/mol Eca for F = -328 kJ/mol E; for K = 418.8 kJ/mol
4) Calculate the lattice enthalpy for calcium fluoride using the Born-Haber cycle method, using the provided...
4) Calculate the lattice enthalpy for calcium fluoride using the Born-Haber cycle method, using the provided table. (Show all your work; 2 points) Enthalpies, AH/(kJ mol) +192 Process Sublimation of Ca(s) Ionization of Ca(g) Dissociation of F2(g) Electron gain by F(g) Formation of CaF (s) +1735 to Ca(ag +157 -328 -1220
Using the Born Haber cycle in the previous question, and the following energies, calculate the standard...
Using the Born Haber cycle in the previous question, and the following energies, calculate the standard energy of formation for Srl2 Enthalpy of sublimation of Sr(s) = 164 kJ/mol 1st ionization energy of Sr(g) = 549 kJ/mol 2nd ionization energy of Sr(g) - 1064 kJ/mol Enthalpy of sublimation of 12(s) = 62 kJ/mol Bond dissociation energy of 12(g) - 153 kJ/mol 1st electron affinity of l(g) = -295 kJ/mol Lattice energy of Srlz(s) = -1960 kJ/mol *Note: Do not include...
Draw the Born-Haber Cycle with these values and calculate lattice energy. Problem 1: Label each reaction...
Draw the Born-Haber Cycle with these values and calculate
lattice energy.
Problem 1: Label each reaction listed below for the Born-Haber cycle in the formation of Cao lattice and calculate the lattice energy of Cal given the following information. AH KD) Ca(s) + Ca(8) 193 Calg) - Cat (8) + e 590 Cat (8) - Cat (8) + e- 2 O(g) + O2(g) O(8) + e- O (8) -141 O (8) + e- O (8) 878 Ca(s) + O2(g) →...
Calculate the net energy change in kilojoules per mole that takes place on formation of BeF2(s) from the elements: Be(s)...
Calculate the net energy change in kilojoules per mole that takes place on formation of BeF2(s) from the elements: Be(s)+F2(g)⟶BeF2(s) The following information is needed: Heat of sublimation for Be(s)= 325.8 kJ/mol Eea for F(g)= −328 kJ/mol Bond dissociation energy for F2(g)= 158 kJ/mol Ei1 for Be(g)= 899.5 kJ/mol Electrostatic interactions in BeF2(s)= −3505 kJ/mol Ei2 for Be(g)= 1757.1 kJ/mol
Using the data given below, sketch a Born-Haber cycle for the formation of BaC2(s) and insert the various equations and energy values into the individual steps of your cycle Sublimation energy fo...
Using the data given below, sketch a Born-Haber cycle for the formation of BaC2(s) and insert the various equations and energy values into the individual steps of your cycle Sublimation energy for Ba(s) +180 kJmol1 Electron affinity for Cl(g)-346 kJmol1 First ionization energy for Ba(g)-+514 kJmol1 Bond dissociation energy for Clh(g) +243 kJmol Enthalpy of formation of BaCl2: Ba(s) + Ch(g) BaCh(s)--610 kJmol Lattice energy. Ba2+(g) + 2Cl.(g) → BaCl2(s)--2075 kJmol-1 Calculate the second ionization energy for Ba+(g) → Ba2+(g)...
Calculate the energy change (in kilojoules per mole) for the formation of the following substances from...
Calculate the energy change (in kilojoules per mole) for the formation of the following substances from their elements. CaF2 (The sublimation energy for Ca is +178.2 kJ/mol, Ei1 = +589.8 kJ/mol, Ei2 = +1145kJ/mol, and the lattice energy of CaF2 is 2630 kJ/mol.) Express the energy change in kilojoules per mole to four significant digits.
Using the thermodynamic quantities shown below: construct a Born-Haber cycle for the following reaction: Li(s) +...
Using the thermodynamic quantities shown below: construct a
Born-Haber cycle for the following reaction: Li(s) + 1/2
F2(g)
LiF(s); calculate the lattice energy of LiF.
Vaporization of Li(s): +159
F2 bond enthalpy: +155
Li ionization energy: +520
F- electron affinity: +328
LiF(s) heat of formation: -616
Calculate the net change in energy in kJ that takes place on formation of 50.44 moles...
Calculate the net change in energy in kJ that takes place on formation of 50.44 moles of MgF2(s) from Mg(s) + F2(g) → MgF2(s) given the following information: Heat of sublimation for Mg(s) = 147.7 kJ/mol Bond dissociation energy for F2(g) = 158 kJ/mol Electrostatic interactions in MgF2(s) = -2957 kJ/mol Eea for F(g) = -328 kJ/mol Ei1 for Mg(g) = 737.7 kJ/mol Ei2 for Mg(g) = 1450.7 kJ/mol
7. Use the Born Haber cycle and the given information to determine the net energy change (in kJ/mol) that takes place in the formation of KF(s) from the elements: Ks) + F2@KFS) Heat of sublimation of K = 89.2 kJ/mol Bond dissociation energy for F2 = 158 kJ/mol Lattice Energy of KF = 821 kJ/mol Eca for F = -328 kJ/mol E; for K = 418.8 kJ/mol
4) Calculate the lattice enthalpy for calcium fluoride using the Born-Haber cycle method, using the provided table. (Show all your work; 2 points) Enthalpies, AH/(kJ mol) +192 Process Sublimation of Ca(s) Ionization of Ca(g) Dissociation of F2(g) Electron gain by F(g) Formation of CaF (s) +1735 to Ca(ag +157 -328 -1220
Using the Born Haber cycle in the previous question, and the following energies, calculate the standard energy of formation for Srl2 Enthalpy of sublimation of Sr(s) = 164 kJ/mol 1st ionization energy of Sr(g) = 549 kJ/mol 2nd ionization energy of Sr(g) - 1064 kJ/mol Enthalpy of sublimation of 12(s) = 62 kJ/mol Bond dissociation energy of 12(g) - 153 kJ/mol 1st electron affinity of l(g) = -295 kJ/mol Lattice energy of Srlz(s) = -1960 kJ/mol *Note: Do not include...
Draw the Born-Haber Cycle with these values and calculate
lattice energy.
Problem 1: Label each reaction listed below for the Born-Haber cycle in the formation of Cao lattice and calculate the lattice energy of Cal given the following information. AH KD) Ca(s) + Ca(8) 193 Calg) - Cat (8) + e 590 Cat (8) - Cat (8) + e- 2 O(g) + O2(g) O(8) + e- O (8) -141 O (8) + e- O (8) 878 Ca(s) + O2(g) →...
Using the data given below, sketch a Born-Haber cycle for the formation of BaC2(s) and insert the various equations and energy values into the individual steps of your cycle Sublimation energy for Ba(s) +180 kJmol1 Electron affinity for Cl(g)-346 kJmol1 First ionization energy for Ba(g)-+514 kJmol1 Bond dissociation energy for Clh(g) +243 kJmol Enthalpy of formation of BaCl2: Ba(s) + Ch(g) BaCh(s)--610 kJmol Lattice energy. Ba2+(g) + 2Cl.(g) → BaCl2(s)--2075 kJmol-1 Calculate the second ionization energy for Ba+(g) → Ba2+(g)...
Using the thermodynamic quantities shown below: construct a
Born-Haber cycle for the following reaction: Li(s) + 1/2
F2(g)
LiF(s); calculate the lattice energy of LiF.
Vaporization of Li(s): +159
F2 bond enthalpy: +155
Li ionization energy: +520
F- electron affinity: +328
LiF(s) heat of formation: -616
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