HomeworkLib
Question

OADVANCED MATERIAL Interpreting a Born-Haber cycle This thermodynamic cycle describes the formation of an ionic compound M X2▼ | 700,- 600 M (g) + 2x (g 500 enthalpy 400. 300. м (е) + x, (g) 200 100. м (s) + X2(g) 0. -100. 200. м Х, (s)DANCED MATERIAL Interpreting a Born-Haber cycle -200. MX What is the lattice enthalpy of MX2? kJ/mol kJ/mol More stable. What

OADVANCED MATERIAL Interpreting a Born-Haber cycle This thermodynamic cycle describes the formation of an ionic compound M X2 from a metal element M and nonmetal element X in their standard states. Use it to answer the questions in the table below. 2+ 1100 1000 900 2- 800--- 700 600 M (8)+2X) 500. enthalpy 400 (kJ/mol) 300. M (g) + X, (g) 200
▼ | 700,- 600 M (g) + 2x (g 500 enthalpy 400. 300. м (е) + x, (g) 200 100. м (s) + X2(g) 0. -100. 200. м Х, (s)
DANCED MATERIAL Interpreting a Born-Haber cycle -200. MX What is the lattice enthalpy of MX2? kJ/mol kJ/mol More stable. What is the formation enthalpy of M X2? Suppose both the X-X bond enthalpy and the heat of sublimation of M were smaller. Would MX2 be more stable? Or less? O Less stable. It is impossible to tell without more information
science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

classmAte Date 2十 ahelecro Enegy qusd 과00 remave electrons o atomuyahon atice ne Erth alpy atorisaha pe MX2 (s) tat ase brougclAssmute Dafe Page 2 1 (-25。 -800)s升w.el 2S0 滸 bose both -thex-X bond etha 팎 sublimat D& to tu--10lthout intornahon , mau lw

0 0
Add a comment
Know the answer?
Add Answer to:
OADVANCED MATERIAL Interpreting a Born-Haber cycle This thermodynamic cycle describes the formati...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • j This thermodynamic cycle describes the formation of an ionic compound M X from a metal...

    j This thermodynamic cycle describes the formation of an ionic compound M X from a metal element M and nonmetal element X in their standard states. Use it to answer the questions in the table below. 900. 2m* () + 2e + x (8) 800. 700. 600. 2M* (x) + x2 (g) 500. 400. 2M (8) + x() enthalpy (kJ/mol 24 (2) + 5x (2) 2M(5) + -,() 1 -100 - 200. M.X(s) What is the lattice enthalpy of M2X...

  • This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M...

    This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Use it to answer the questions in the table below 900 800 700 600 + X enthalpy 400 300. 200. 100. 0. 100.- kJ/mol M3 What is the lattice enthalpy of MX? 1 kJ/mol What is the enthalpy of formation of MX?kJ/mol Suppose both the heat of sublimation of M and the electron affinity of X...

  • Question 4 4 pts Use the Born-Haber Cycle to calculate the lattice energy for the formation...

    Question 4 4 pts Use the Born-Haber Cycle to calculate the lattice energy for the formation of X2Y. Input your answer in units of kJ/mole with the correct sign. Process Enthalpy (kJ/mol). X(s)--> X(g) 115 X(g) -->X*(8) + le 499 Y2 (8) --> 2Y (8) 264 -295 Y (8) + 1e.-->Y (8) Y (8) + 1e' --> Y2 () 115 2X(s) +% Y2 (8)--> X2Y(s) -549

  • 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...

  • 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

  • 1)a. Using the Born Haber cycle, determine the enthalpy for lattice formation of MgO. Mg (s),...

    1)a. Using the Born Haber cycle, determine the enthalpy for lattice formation of MgO. Mg (s), ΔHsub = +148 kJ/mol bond dissociation energy for O2 = +499 kJ/mol 1st ionization energy for Mg = +738 kJ/mol    1st electron affinity for O = –141 kJ/mol 2nd ionization energy for Mg = +1450 kJ/mol 2nd electron affinity for O = +844 kJ/mol MgO(s), enthalpy of formation = –602 kJ/mol 1)b. Calculate the lattice formation energy of MgO using the Madelung constant....

  • Physical Chemistry: Use a Born-Haber cycle to find an experimentally based value for the lattice enthalpy...

    Physical Chemistry: Use a Born-Haber cycle to find an experimentally based value for the lattice enthalpy of sodium bromide (NaBr(s)). The lattice enthalpy corresponds to the enthalpy change for the process NaBr(s) rightarrow Na^+(g) + Br^-(g) Use the following information in doing this problem. delta H degree_f(Na(g)) = 107.32 kJ/mol delta H degree_IE1(Na(g)) = 495.8 kJ/mol delta H degree_f(Br(g)) = 111.88 kJ/mol delta H degree_EA(Br(g)) = -324.6 kJ/mol delta H degree_f(NaBr(s)) = -361.06 kJ/mol The ionization enthalpy (IE_1) and electron...

  • Born-Fajans-Haber Cycle Suppose a chemist discovers a new metallic element and names it "Xtrinsium" (Xt) Xt...

    Born-Fajans-Haber Cycle Suppose a chemist discovers a new metallic element and names it "Xtrinsium" (Xt) Xt exhibits chemical behaviour similar to an alkaline earth Xt(s) + Cl2(g) → XtCl2(s) Lattice energy for XtCl2 First Ionization energy of Xt Second Ionization energy of Xt Electron affinity of Cl Bond energy of Cl2 Enthalpy of sublimation (atomization) of Xt 2260. kJ/mol 430. kJ/mol 731 kJ/mol -348.7 kJ/mol 239 kJ/mol 170. kJ/mol Use the above data to calculate ΔHof for Xtrinsium chloride.

  • 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

  • 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

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT