Question

Calculate the energy of electrostatic attractions of LiCl(s). The following information is needed. Heat of sublimation...

Calculate the energy of electrostatic attractions of LiCl(s). The following information is needed.

Heat of sublimation for Li(s)= 161 kJ/mol Eea for Cl(g)= −349 kJ/mol
Bond dissociation energy for Cl2(g)= 243 kJ/mol Ei for Li(g)= 520 kJ/mol
Li(s)+12Cl2(g)→LiCl(s)ΔE= −409 kJ/mol
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Given the following information: Energy of sublimation of K(s) = 77 kJ/mol Bond energy of HCl...
Given the following information: Energy of sublimation of K(s) = 77 kJ/mol Bond energy of HCl = 427 kJ/mol Ionization energy of K(g) = 419 kJ/mol Electron affinity of Cl(g) = –349 kJ/mol Lattice energy of KCl(s) = –705 kJ/mol Bond energy of H2 = 432 kJ/mol Calculate the net change in energy for the following reaction: 2K(s) + 2HCl(g) → 2KCl(s) + H2(g) ΔE = ______ kJ
Given the following information: Li(s) → Li(g) enthalpy of sublimation of Li(s) = 166 kJ/mol HF(g)...
Given the following information: Li(s) → Li(g) enthalpy of sublimation of Li(s) = 166 kJ/mol HF(g) → H(g) + F(g) bond energy of HF = 565 kJ/mol Li(g) → Li+(g) + e– ionization energy of Li(g) = 520. kJ/mol F(g) + e– → F–(g) electron affinity of F(g) = -328 kJ/mol Li+(g) + F–(g) → LiF(s) lattice energy of LiF(s) = -1047 kJ/mol H2(g) → 2H(g) bond energy of H2 = 432 kJ/mol Calculate the change in enthalpy for: 2Li(s)...
te the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kJ/mol ∆Hf...
te the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kJ/mol ∆Hf for F(g) +77 kJ/mol first ionization energy of Li(g) +520. kJ/mol electron affinity of F(g) –328 kJ/mol enthalpy of formation of LiF(s) –617 kJ/mol A. none of these B. –650. kJ/mol C. 285 kJ/mol D. 800. kJ/mol E. 1052 kJ/mol
Use the Born Haber cycle (show relevant steps) to determine the lattice energy of CsCl (s)...
Use the Born Haber cycle (show relevant steps) to determine the lattice energy of CsCl (s) from the following data: Hf 0 [CsCl(s)] = -442.8 kJ/mol; enthalpy of sublimation of Cesium is 78.2 kJ/mol; enthalpy of dissociation of Cl2 (g) = 243 kJ/mol Cl2 ; IE1 for Cs(g) = 375.7 kJ/mol; electron affinity enthalpy-EA1 for Cl(g) = -349kJ/mol. - need answer fast - thanks
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the heat of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
Calculate the second ionization energy of the metal M (ΔHion2° in kJ/mol) using the following data:...
Calculate the second ionization energy of the metal M (ΔHion2° in kJ/mol) using the following data: Lattice enthalpy of MO(s), ΔHl° = -2297 kJ/mol Bond dissociation enthalpy of O2(g) = +498 kJ/mol First electron affinity of O = -141 kJ/mol Second electron affinity of O = +744 kJ/mol Enthalpy of sublimation of M = + 102 kJ/mol First ionization energy of M = + 340 kJ/mol Standard enthalpy of formation of MO(s), ΔHf° = -336 kJ/mol Refer to the textbook...
Use the Born-Haber cycle, and the following data to calculate the bond dissociation energy of F2....
Use the Born-Haber cycle, and the following data to calculate the bond dissociation energy of F2. Na(g) → Na+(g) + e-(g)    ΔrH = IE1 = 500 kJ mol-1 Na(s) → Na(g)    ΔsubH = 107 kJ mol-1 F-(g) → F(g) + e-(g)    ΔrH = EA1 = 329 kJ mol-1 Na(s) + 1/2 F2(g) → NaF(s)    ΔfH = -569 kJ mol-1 Na+(g) + F-(g) → NaF(s)    ΔlattH = -928 kJ mol-1
1-Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of...
1-Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: Round your answer to zero decimal places. N2(g)+3H2(g)---2NH3(g) Round your answer to zero decimal places. 2-Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: →+4H2O2lPbSs+PbSO4s4H2Ol Round your answer to zero decimal places. substance Δ Hf ° (kJ/mol) Δ Gf ° (kJ/mol) S ° (J/mol∙K) Aluminum Al3+ (aq) --- -485.0 ---...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT