HomeworkLib
Question

#1.Calculate ∆solnH (kJ/mol) when lithium chloride is added to water. #2.Given that K = 3.07 for...

#1.Calculate ∆solnH (kJ/mol) when lithium chloride is added to water.

#2.Given that K = 3.07 for the reaction C(s,graphite)+ CO2(g) ↔ 2 CO(g) at 652 °C, determine the Gibbs reaction energy (in kJ mol-1) at 652 °C.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Doll will be negative as heat will be released. Exact value can be calculated using Al=MCAT specific heat of water = 4.18 Jg

0 0
Add a comment
Know the answer?
Add Answer to:
#1.Calculate ∆solnH (kJ/mol) when lithium chloride is added to water. #2.Given that K = 3.07 for...
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

  • Given that K = 3.83 for the reaction C(s,graphite)+ CO2(g) ↔ 2 CO(g) at 606 °C,...

    Given that K = 3.83 for the reaction C(s,graphite)+ CO2(g) ↔ 2 CO(g) at 606 °C, determine the Gibbs reaction energy (in kJ mol-1) at 606 °C.

  • Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the...

    Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the reaction of dissolving silver sulfide, Ag2S, in water (25 C.) Do the calculations in two ways. Use the standard Enthalpy of formation, deltaH, and entropy S values, and the formula deltaG=deltaH-TdeltaS. Use the standard free energies of formation deltaG and the formula deltaG=deltaG(products)-deltaG(reactants).

  • 1--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? CH4 (g)...

    1--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? CH4 (g) + 2 O2 (g) ⇌ CO2 (g) + 2 H2O (g) The conditions for this reaction are: PCH4 = 0.73 bar PO2 = 0.27 bar PCO2 = 0.10 bar PH2O = 1.41 bar 2--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 =...

  • Using the following data determine the temperature (in K) at which the reaction H2O(g)+ C(s,graphite) ↔...

    Using the following data determine the temperature (in K) at which the reaction H2O(g)+ C(s,graphite) ↔ H2(g) + CO(g) this becomes spontaneous. ΔfH° (H2O(g)) = -251.2 kJ mol-1 ΔfH° (C(s,graphite)) = 0.0 kJ mol-1 ΔfH° (H2(g)) = 0.0 kJ mol-1 ΔfH° (CO(g)) = -110.1 kJ mol-1 S° (H2O(g)) = 192.6 J K-1 mol-1 S° (C(s,graphite)) = 6.4 J K-1 mol-1 S° (H2(g)) = 136.9 J K-1 mol-1 S° (CO(g)) = 192.4 J K-1 mol-1

  • 5. The standard molar entropy of liquid ethanol (C2H5OH) is 160.7 J K mol and the...

    5. The standard molar entropy of liquid ethanol (C2H5OH) is 160.7 J K mol and the standard enthalpy of combustion is - 1368 kJ mol at 298 K, how much is the standard Gibbs energy (A,Gº) of formation of liquid ethanol at 298 K? (20 pts) The formation reaction of ethanol is 2C (graphite) + O2(g) + 3H2 (g) → C2H5OH() The combustion reaction of ethanol is CH5OH (1) + 302 (9) ► 200, (g) + 3H20 (1) CO; (g)...

  • Use Hess's law to determine Ofor the reaction → CO2(g),given that C(graphite) +202(8) — CO(8) A Hº = -110.54 kJ mol C(g...

    Use Hess's law to determine Ofor the reaction → CO2(g),given that C(graphite) +202(8) — CO(8) A Hº = -110.54 kJ mol C(graphite) + O2(8) —CO2(g) A Hº = -393.51 kJ mol

  • Part I. Use a Born-Haber cycle to calculate the lattice energy of KCl from the following...

    Part I. Use a Born-Haber cycle to calculate the lattice energy of KCl from the following data. (5 marks) Ionization energy of K(g) = 444.0 kJ mol-1 Electron Affinity of Cl(g) = -381.0 kJ mol-1 Energy to Sublime K(s) = 152.0 kJ mol-1 Bond energy of Cl2 = 201.0 kJ mol-1 ∆rH for K(s) + 1/2 Cl2(g) ↔ KCl(s) = -480.0 kJ mol-1 art II. Using the lattice energy calculated in part I determine the enthalpy of solution potassium chloride...

  • answers ncider 31. The work function for lithium is 279.7 KJ/mol. a. What is the maximum...

    answers ncider 31. The work function for lithium is 279.7 KJ/mol. a. What is the maximum wavelength of light that can remove an electron from an atom on the surface of lithium metal? 5/3 ly 32. Given the following data: A. Pa(s) + 6 Cl:(g)4 PCl(g) B. Pa(s)+ 5 0:(g) P4Oo(s)AH-2967.3 C. PCl(g) + Cl:(g) PCls(g) D. PCIb(g)+%O:(g) ClaPO(g) AH-1225.6 kJ 3ot AH-84.2 AH-285.7 Calculate AH for the reaction: P4O10(s)+6 PCIs(g) 10 ClhPO(g). Note when I solved this problem, I...

  • AH-116.4 kJ/mol 4. Consider the following reaction: NH.NO, (s) N20 (8) + 2 H20 (g) Calculate...

    AH-116.4 kJ/mol 4. Consider the following reaction: NH.NO, (s) N20 (8) + 2 H20 (g) Calculate AGⓇ for the reaction. Substance S” (J/mol K) NH.NO, (3) 151 N:0 (8) 220 H:0 (9) 183 5. The first step in the commercial production of titanium metal is the reaction of Tio: with chlorine an graphite: TiO2 (s) + 2 Cl: (g) + 2C (5) Tici: (1) + 2 CO(g) Calculate AGº for the reaction. Substance AG? (kJ/mol Substance AG® (kJ/mol) C(s) TiCl...

  • 1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8...

    1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous 2. Consider a...

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