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want to check 4 5 and 6 (4) KNO; (s) can be dissolved in water. The...
1. 18 g of LiCl(s) is dissolved in 18.0mL of water that is initially 20.0°C. a) Write the chemical equation for the dissolution of LiCl(s) b) Calculate the molar enthalpy of dissolving LiCl(s) in water. Is this process endothermic or exothermic? c) Calculate the amount of heat absorbed/released when 1.18 g of LiCl(s) dissolves. d) Calculate the final temperature of the solution. You can assume the heat capacity of solution is equal to the heat capacity of water (dwater =...
The salt potassium hydroxide dissolves in water according to the reaction: KOH(s) K+(aq) + OH-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: KOH(s) = -424.8 kJ mol-1 K+(aq) = -252.4 kJ mol-1 OH-(aq) = -230.0 kJ mol-1 kJ (b) Calculate the temperature reached by the solution formed when 8.05 g of KOH is dissolved in 0.162 L of water at 21.8 °C. Approximate the heat capacity of the solution by the heat capacity...
Prepare yourself for the laboratory: Question #2 1.26 g of LiCl(s) is dissolved in 25.0 mL of water that is initially 21.0°C a) Write the chemical equation for the dissolution of LiCl(s) b) Using the thermodynamic tables in Appendix II of Tro, calculate the molar enthalpy of dissolving LiCI(s) in water. Is this process endothermic or exothermic? Calculate the amount of heat absorbed/released when 1.26 g of Licl(s) dissolves. c) d) Calculate the final temperature of the solution. You can...
Instant hot packs contain a solid and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dissolves, increasing the temperature because of the exothermic reaction. The following reaction is used to make a hot pack: LiCl(s)⟶Li+(aq)+Cl−(aq)ΔH=−36.9kJ What is the final temperature in a squeezed hot pack that contains 20.3 g of LiCl dissolved in 112 mL of water? Assume a specific heat of 4.18 J/(g⋅∘C)for the solution, an initial temperature of 25.0 ∘C, and...
The salt copper(II) sulfate dissolves in water according to the reaction: CuSO4(s) ----->Cu2+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: CuSO4(s) = -771.4 kJ mol-1 Cu2+(aq) = 64.8 kJ mol-1 SO42-(aq) = -909.3 kJ mol-1 ______kJ (b) Calculate the temperature reached by the solution formed when 18.3 g of CuSO4 is dissolved in 0.195 L of water at 24.2 °C. Approximate the heat capacity of the solution by the heat capacity...
The salt ammonium chloride dissolves in water according to the reaction: NH4Cl(s) NH4+(aq) + Cl-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: NH4Cl(s) = -314.4 kJ mol-1 NH4+(aq) = -132.5 kJ mol-1 Cl-(aq) = -167.2 kJ mol-1 kJ (b) Calculate the temperature reached by the solution formed when 35.3 g of NH4Cl is dissolved in 0.160 L of water at 24.6 °C. Approximate the heat capacity of the solution by the heat capacity...
The salt cesium perchlorate dissolves in water according to the reaction: CsClO4(s) Cs+(aq) + ClO4-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: CsClO4(s) = -443.1 kJ mol^-1 Cs^+(aq) = -258.3 kJ mol^-1 ClO4-(aq) = -129.3 kJ mol^-1 _____kJ (b) Calculate the temperature reached by the solution formed when 30.0 g of CsClO4 is dissolved in 0.119 L of water at 23.0 °C. Approximate the heat capacity of the solution by the heat capacity...
KNO3(s) is soluble in water and the temperature of the solution decreases as dissolution occurs. Which of the following statements most likely applies to this system? a) The dissolution is exothermic with a favorable entropy change. b) The dissolution is exothermic with an unfavorable entropy change. c) The dissolution is endothermic with a favorable entropy change. d) The dissolution is endothermic with an unfavorable entropy change. e) None of the above.
The salt cesium sulfate dissolves in water according to the reaction: Cs2SO4(s) = 2Cs+(aq) + SO42-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: Cs2SO4(s) = -1443.0 kJ mol-1 Cs+(aq) = -258.3 kJ mol-1 SO42-(aq) = -909.3 kJ mol-1 (b) Calculate the temperature reached by the solution formed when 136 g of Cs2SO4 is dissolved in 0.122 L of water at 22.4 °C. Approximate the heat capacity of the solution by the heat capacity...
Instant cold packs used to treat athletic injuries contain solid NH4NO3 and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dissolves, lowering the temperature because of the endothermic reaction NH4NO3(s)+H2O(l)→NH4NO3(aq) ΔH= +25.7 kJ. What is the final temperature in a squeezed cold pack that contains 43.5 g of NH4NO3 dissolved in 125 mL of water? Assume a specific heat of 4.18J/(g⋅∘C) for the solution, an initial temperature of 29.0 ∘C, and no heat...