I know this is a big one but I've tried and gotten it wrong 4 times and this is my last attempt. Thanks in advance!
I know this is a big one but I've tried and gotten it wrong 4 times...
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 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...
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...
T U IF I question. The salt potassium bromide dissolves in water according to the reaction: KBr(s) + (aq) + Br"(aq) (a) Calculate the standard enthalpy change AH for this reaction, using the following data: AH?KBr(s) --393.8 kJ mol! AHK (aq) --252.4 kJ mol! AH Br"(aq) --121.6 kJ mol' (b) Calculate the temperature reached by the solution formed when 53.9 g of KBr is dissolved in 0.149 L of water at 22.9 °C. Approximate the heat capacity of the solution...
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...
The salt ammonium chloride dissolves in water according to the reaction: NH_CI) —NH4+ (aq) + Cl(aq) (a) Calculate the standard enthalpy change AH° for this reaction, using the following data: AH NHACI() = -314.4 kJ mol-1 AHNH4+(aq) = -132.5 kJ mol-1 AH; Cr(aq) = -167.2 kJ moll kJ (b) Calculate the temperature reached by the solution formed when 36.8 g of NH4Cl is dissolved in 0.186 L of water at 23.7 °C. Approximate the heat capacity of the solution by...
5g CaCl2 100.74 10g CaCl2 100.74 15g CaCl2 100.74 5g NH.CI 100.74 5g Mass of water (g) 10g NH.CI 100.74 10g 15g NH4Cl 100.74 5g 15g Mass of salt (g) Moles of salt (g x mol/g) Initial Temperature (°C) .045 .90 .135 26 26 26 18 18 Final Temperature (°C) 46 14 12 10 8 167.2 585.2 1254 -83.6 -250.8 -501.6 Change in Temperature (°C) AT = T- Heat absorbed by the solution (J) Slx = -(Sw.X mxX AT] Heat...
The salt ammonium perchlorate dissolves in water according to the reaction: NH4ClO4(s) NH4+(aq) + ClO4-(aq) (a) Calculate the standard enthalpy change ΔH° for this reaction, using the following data: NH4ClO4(s) = -295.3 kJ mol-1 NH4+(aq) = -132.5 kJ mol-1 ClO4-(aq) = -129.3 kJ mol-1 kJ (b) Calculate the temperature reached by the solution formed when 33.9 g of NH4ClO4 is dissolved in 0.196 L of water at 23.4 °C. Approximate the heat capacity of the solution by the heat capacity...
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s) → NH(aq) + NO3 (aq) In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C and the final temperature (after...