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Briefly describe how to find the values for both enthalpy and entropy of dissolution from the linear equation.
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- Two students prepared aqueous solutions of LiCl and measured the properties, as shown in the table above. Both students observed that the solid LiCl readily dissolved in H2O. The students drew particle diagrams to explain the changes in the enthalpy and entropy of dissolution for LiCl based on their results and observations. Based on this information, the better particle diagram was drawn by which student, and why is that diagram more accurate? (see attached image) a.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+ and Cl− ions causing an increase in entropy. b.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+and Cl−ions indicating that the dissolution of LiCl is exothermic. c.) The better particle diagram was drawn by Student 2 because it shows that LiCl does not dissociate, resulting in a decrease in entropy for the dissolution of LiCl.…Briefly describe how the values for both enthalpy and entropy of dissolution were determinedfrom the linear equation16) Dissolving of a salt a) Determine whether ammonium nitrate (NH4NO3) will dissolve in distilled water at a temperature of 30 °C or not by calculating the Gibbs energy for this process. In your calculation, use the enthalpy and entropy values given in the table below. b) Using the results from a), calculate the theoretical temperature limit for dissolving NH4NO3 in distilled water. Compound NH4NO3 (S) NH4+ (aq) NO3- (aq) Enthalpy / kJ mol-¹ -365 -130 -204 Entropy / J mol-¹ K-1 150 115 145
- The Gibbs energy of a pure substance is identical to another thermodynamic quantity: the chemical potential, . How does the chemical potential of liquid water relate to the chemical potential of solid ice at standard pressure (1 bar)? How does this change at high pressure? Does the rate at which the wire moves through the ice depend on the amount of weight placed on the wire? If so, how? Consider whether or not this is an equilibrium process. Does it matter how thick the wire is? If so, why? Does it matter if the wire can conduct heat? If so, why?Why is it reasonable to set the chemical potential of a pure liquid or of a pure solidequal to its standard state value , independent of the pressure?The decomposition of a generic diatomic element in its standard state is represented by the equation....
- Calculate the standard Gibbs free energy in kJ mol–1.The standard state of a substance used to be defined as 1 atm at the specified temperature. By how much does the current definition of standard chemical potential (at 1 bar) differ from its former value at 298.15 K?For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A mixture of xenon (Xe) gas and hydrogen (H₂) gas at 2 atm and 48°C. 300 mL of a solution made from ammonium iodide (NH4I) dissolved in water. A solution made of ammonium iodide (NH I) in water, at 58°C. Change An additional 2.0 L of pure H₂ gas is added to the mixture, with the pressure kept constant at 2 atm. 0.5 g of NH I crystallizes out of the solution, without changing the temperature. 50. mL of pure water is added to the solution. AS ⒸAS 0 not enough information AS 0 not enough information AS 0 not enough information ? 00. 18 Ar BA Ò
- 1. Briefly distinguish between spontaneity criteria of simple and non-simple system in terms of Gibbs and Helmholtz free energies.Why does the dissolution of MgCl2 have a negative entropy value?(a) In the lab, you have just prepared an unknown product, and you wish to characterize its physical properties. You find that its vapor pressure is 0.386 bar at 400 K, and that its normal boiling point is 432 K. Use the Clausius-Clapeyron equation to estimate the value of AvapH for this compound in kJ. (b) With the information you have accumulated in part (a), now evaluate the molar entropy change, AvapS, for vaporization of your product, in J/K. (c) The vapor pressure of solid 12 (iodine) is given by 8090.0 K 2.013 ln(T) + 32.908 T where P is in atm and T is in K. Use this equation to compute the normal sublimation temperature, Tsubl (in K). (Note: It is best to use WolframAlpha or some numerical method, such as a Newton-Raphson iteration, to find the solution for this problem.) In(P) =
