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The following data compare the standard enthalpies and free energies of formation of some crystalline ionic substances and aqueous solutions of the substances:
(a) Write the formation reaction for AgNO3(s). Based on this reaction, do you expect the entropy of the system to increase or decrease upon the formation of AgNO3(s)?
(b) Use ?H°f and ?G°f of AgNO3(s) to determine the entropy change upon formation of the substance. Is your answer consistent with your reasoning in part (a)?
(c) Is dissolving AgNO3 in water an exothermic or endothermic process? What about dissolving MgSO4 in water?
(d) For both AgNO3 and MgSO4, use the data to calculate the entropy change when the solid is dissolved in water. (e) Discuss the results from part (d) with reference to material presented in this chapter and in the "A Closer Look" box on page 540.
Write the charge balance eqtn for a saturated soln of CdCO3. Hint: there are 4 relevent chemical eqtns
Draw the condensation reaction that would form the dipeptide Met-Ile from the amino acids, Methionine and Isoleucine. Based on the characteristics of the side chains ONLY, would you expect the dipeptide to be polar or nonpolar
An open-end manometer containing mercury was connected to a vessel holding a gas at a pressure of 850torr. The atmospheric pressure was 630torr. Explain what is the difference in the heights of the mercury expressed in cm
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ethylene oxide polyol that has been generated from pentaerythritol with hexamethylene di-isocyanate, where the ratio of hydroxyl groups to isocyanate groups
1) Determine the change in entropy for the expansion of 0.10 mole of an ideal gas from 2.0L to 3.0 L at constant temperature? My work: 0.10 mole * (8.314 J/K)/ (1 mole) * ln (3.0L/2.0L) = 0.33 J/K
A sample of nitrogen has a volume of 605 mL at a pressure of 84.77 kPa. Assuming that the temperature is constant, at what pressure will the gas has a volume of 0.766 L
What is theb Kp equalibrium constant expression for the following equalibrium? S8 (s) + 24F2(g) 8SF6(g) Kp=
After adding the two portions of water into your calorimeter setup and following the procedure outlined in the experiment, you determine the temperature of the mixed portions of water to be 45 oC. What is the heat capacity of the calorimeter
Calculate the conditional formation constant Kf for the formation of an EDTA complex with copper (II) at a pH of 5.00, if log Kf= 18.80
A 388 mL container holds 0.146 g of Ne and an unknown amount of Ar at 35°C and a total pressure of 640. mmHg. Calculate the moles of Ar present.
The mass of the final solution is 73.0 grams, and its heat capacity is 3.85 J/g°C; the heat capacity of the calorimeter is 5.0 J/°C. Calculate the Hreaction in kJ/mol metal.
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