The dissolution of NH4CIO4(s) in water is endothermic, with +33.5 kJ/mol. If you prepare a 1.00 m solution of AHsoln = NH,CIO4 beginning with water at 25.0 °C, what is the final tem- perature of the solution in °C? Assume that the specific heats of both pure H2O and the solution are the same, 4.18 /(K•g).

The dissolution of NH4CIO4(s) in water is endothermic, with +33.5 kJ/mol. If you prepare a 1.00 m solution of AHsoln = NH,CIO4 beginning with water at 25.0 °C, what is the final tem- perature of the solution in °C? Assume that the specific heats of both pure H2O and the solution are the same, 4.18 /(K•g).

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.96PAE: 9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in...

See similar textbooks

Similar questions

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.)
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.
5.61 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
3.56 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
7.16 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. A 44.0 g sample of an unknown metal at 100.0 °C is placed in a constant pressure calorimeter containing 80.0 g of water at 24.8 °C. The final temperature is 28.4 °C. Assume that the heat capacity of the calorimeter equals the heat capacity of the water it contains. Calculate the specific heat capacity of the metal and use the result to identify the metal.
Calculate the enthalpy of solution for the dissolution of lithium iodide, LiI, molar mass = 133.85 g mol-1. When 1.49 g of LiI is dissolved in a coffee cup calorimeter containing 75.0 mL of water the temperature increased from 23.5 °C to 25.7 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1. -62 kJ mol-1 -39 kJ mol-1 30 kJ mol-1 -76 kJ mol-1 18 kJ mol-1
A 5.00 g-sample of KOH at 25.0 C was added to 100.0 g of H2O(l) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH is a thermodynamically favorable process? A. The forces between the ions and the water molecules are stronger than the forces between water molecules, thus, delta H < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus delta S > 0. Therefore, delta G < 0. B. The energy require to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus delta H < 0. Also, the ions become widely dispersed as KOH(s) dissolved, thus delta S > 0. Therefore, delta G < 0. C. The average kinetic energy of the particles increases, resulting in delta H > 0. Also, the…
When 4.20 g of solid NH4NO3 dissolves in 50.0 g of water at 26.8°C in a calorimeter, the temperature decreases to 20.9°C. The value of q for this reaction is 1.34 kJ. Calculate the enthalpy of solution (ΔH for the dissolution) in kilojoules per mole of NH4NO3 under the given conditions. (Assume that the specific heat of the aqueous solution is the same as water, 4.180 J/g·°C, and not sensitive to temperature over the temperature range.)
The answer to the question in the picture is 217 kJ. For the reaction given in Part A, ΔS∘rxnΔSrxn∘ is 25.0 J/KJ/K . What is the standard Gibbs free energy of the reaction, ΔG∘rxnΔGrxn∘?
. Find the maximum possible temperature that may bereached when 0.050 mol Ca(OH)2(s) is allowed to reactwith 1.0 L of a 1.0-M HCl solution, both initially at 25°C.Assume that the final volume of the solution is 1.0 L, andthat the specific heat at constant pressure of the solutionis constant and equal to that of water, 4.18 J K-1g-1.
Calculate the amount of salt in a commercial cold-pack containing ammonium nitrate (ΔHsol = + 25.7 kJ/mol) if the final temperature of the cold-pack is 3ºC. Assume that the initial temperature of water is 25ºC, mass of solution is 25 g and the specific heat of the solution is 4.184 J/g.K.
The quantity of 83.0 g of potassium iodide (KI) is added to water to give a solution with a mass of 150. g. Assume that this solution is very dilute and thus has the same heat capacity as water. The dissolution reaction and the associated heat for potassium iodide is KI (s) -→ K+(aq) + I-(aq) qrx = DHrx = +20.3 kJ. Calculate the change in the temperature of the solution.