Plot your values of In(Ksp) VS. 1/T and find the slope and y-intercept of the best fit line. Use the equation for the best fit line and the following equation ΔΗ AS In(К) %3D RT R to calculate AH and ASº for dissolving Borax What is the slope of your best fit line in the plot? What is ΔΗ (J/mol)? What is the y-intercept of your best fit line in the plot?

Plot your values of In(Ksp) VS. 1/T and find the slope and y-intercept of the best fit line. Use the equation for the best fit line and the following equation ΔΗ AS In(К) %3D RT R to calculate AH and ASº for dissolving Borax What is the slope of your best fit line in the plot? What is ΔΗ (J/mol)? What is the y-intercept of your best fit line in the plot?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.57PAE: Calculate G for the dissolution of both sodium chloride and silver chloride using data from Appendix...

See similar textbooks

Similar questions

The following reaction occurs in pure water: H2O(l)+H2O(l)H3O+(aq)+OH-(aq) which is often abbreviated as H2O(l)H+(aq)+OH-(aq) For this reaction, G = 79.9 kJ/mol at 25C. Calculate the value of G for this reaction at 25C when [OH] = 0.15 M and [H+] = 0.71 M.
Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
Calculate G for the dissolution of both sodium chloride and silver chloride using data from Appendix E. Explain how the values you obtain relate to the solubility rules for these substances.
9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
Calculate ∆Gº for the following reaction at 25ºC: Pb2+ + Fe --> Pb + Fe2+ -->
When solutions containing silver ions and chloride ions aremixed, silver chloride precipitatesAg+(aq) + Cl-(aq) ------> AgCl(s) ΔH = -65.5 kJ(a) Calculate ΔH for the production of 0.450 mol of AgCl bythis reaction. (b) Calculate ΔH for the production of 9.00 gof AgCl. (c) Calculate ΔH when 9.25 x 10-4 mol of AgCl dissolvesin water.
Researchers working on a Lake measured the following in the anoxic bottom waters:[Fe2+] = 100 μM and [S2-] = 50 fM (femtomolar). The formation of FeS(s)Fe2+ + S2- is an important controlling reaction for the solubilityof Fe(+II) under anoxic conditions. In this lake, the temperature at the bottom is about 10°C inthe summer.a. Calculate Kideal for this reaction, ignoring non-idealities.b. Correct K for the temperature at the lake bottom.c. Is the lake water at equilibrium with FeS(s) in the aquifer? If not, given more time,would more solid dissolve or precipitate?
For the reaction: CuS (s) + H₂(g) → H₂S (g) + Cu (s) Given: ΔS ⁰ (CuS) = 66.5 J/mole-K ΔHf ⁰ (CuS) = -53.1 kJ/mol ΔS ⁰ (H₂S) = 205 J/ mole-K ΔHf ⁰ (H₂S) = -20.6 kJ/mol ΔS ⁰ (Cu) = 33.3 J/ mole-K ΔH f ⁰ (Cu) = 0.0 kJ/mol ΔS ⁰ (H₂) = 131 J/ mole-K ΔH f ⁰(H₂) = 0.0 kJ/mol The standard free energy of the reaction ΔG ⁰ rxn is A) -37.9 kJ/mole B) 44.6 kJ/mole C) -20.3 kJ/mole D) +20.3kJ/mole and spontaneous E) +37.9 kJ/mole
Calculate the Enthalpy of change in Kj/mol and % difference in the neutralization reaction below: HNO2 + NH3 = N2 + 2 H2O Initial Temp= 20 Deg celsius Final Temp= 22.3 Deg celsius Conc= 0.4 M [HNO3] and 0.4 M [NH3] Vol= 55 mL [HNO2] and 60 mL [NH3]= Mass is 115 g Specific Heat= 4.184 J/g For the other value in % difference use: -348 Kj/mol
A 5.00 g sample of an unknown salt is dissolved in 50.0 mL of water. During dissolution, the temperature of the solution increases from 24.53 oC to 26.82 oC. Which statement(s) is(are) true? qsurroundings > 0 qsystem < 0 qsystem > 0 qsurroundings < 0 (You can choose more than one)