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Question 7 of 16 > In a calorimeter, 1.045 g of an unknown salt is dissolved...
Assuming that the specific heat of the solution is 4.18 J/(g⋅∘C) and that the calorimeter itself...
Assuming that the specific heat of the solution is 4.18
J/(g⋅∘C) and that the calorimeter itself absorbs a negligible
amount of heat, calculate ΔH in kilojoules for the reaction.
Part A Assuming that the specific heat of the solution is 4.18 J/(g . C) and that the calorimeter itself absorbs a negligible amount of heat, calculate AH in kilojoules for the reaction K2O(8)+H20()-2KOH(aq) ανα ΑΣφ ? ΔΗ - kJ Request Answer Submit Provide Feedback Next> Constants Periodic Tab When 1.045...
8 4 points When a 0.456 g sample of salt is dissolved into water in a...
8 4 points When a 0.456 g sample of salt is dissolved into water in a completely insulated calorimeter (a simple styrofoam coffee cupl. the temperature of the 500 ml water decreases by 0.940°C. What is the heat for the system (the salt dissolving)? O 1.79kJ 0 +1.80 kJ O +214) O 0.214 - 1.96 kJ +1.97 Ooo
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water...
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water at 25.0 oC. The temperature in the calorimeter is measured to be 39.2 oC when the dissolution of CaCℓ2 is completed. Assuming that the specific heat of solution is equal to that of water, i.e., 4.184 J/g oC, calculate the heat of solution of CaCℓ2 in water, in kJ/mol.
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water...
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water at 25.0 oC. The temperature in the calorimeter is measured to be 39.2 oC when the dissolution of CaCℓ2 is completed. Assuming that the specific heat of solution is equal to that of water, i.e., 4.184 J/g oC, calculate the heat of solution of CaCℓ2 in water, in kJ/mol.
The salt sodium perchlorate is soluble in water. When 9.07 g of NaClO4 is dissolved in...
The salt sodium perchlorate is soluble in water. When 9.07 g of NaClO4 is dissolved in 103.00 g of water, the temperature of the solution decreases from 25.00 to 22.70 °C. Based on this observation, calculate the enthalpy of dissolution of NaClO4 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution kJ/mol =
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water...
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water at 25.0 oC. The temperature in the calorimeter is measured to be 39.2 oC when the dissolution of CaCℓ2 is completed. Assuming that the specific heat of solution is equal to that of water, i.e., 4.184 J/g oC, calculate the heat of solution of CaCℓ2 in water, in kJ/mol. final answer is :-29.6
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water at 25.0 oC. The temperature in...
In a coffee-cup calorimeter, 11.0-g sample of solid CaCℓ2 is dissolved in 125 g of water at 25.0 oC. The temperature in the calorimeter is measured to be 39.2 oC when the dissolution of CaCℓ2 is completed. Assuming that the specific heat of solution is equal to that of water, i.e., 4.184 J/g oC, calculate the heat of solution of CaCℓ2 in water, in kJ/mol.
The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, th...
The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, the temperature of the solution decreases from 25.00 °C to 22.56 °C. Based on this observation, calculate the dissolution enthalpy, ΔdissH, of CsCl. Assume that the specific heat capacity of the solution is 4.184 J g-1 °C-1 and that the energy transfer to the calorimeter is negligible. ΔdissH = kJ/mol
Please help how to solve this question An unknown metal weighting 13.11 g at a temperature...
Please help how to solve this question An unknown metal weighting 13.11 g at a temperature of 81.0 degrees Celius is place in a calorimeter containing 25.0 mL of water at a temperature of 25.0 degrees Celsius. The final equilibrium temperature is 30.0 degrees Celius. What s the specific heat of the metal? The specific heat of water is 4.184 J/g-C. Assume the density of water is 1.00g/mL and that there is no heat lost or gained by the calorimeter.
When 3.90 g of cesium perchlorate (CsClO4) is dissolved in 112 g of water in a...
When 3.90 g of cesium perchlorate (CsClO4) is dissolved in 112 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 22.93 °C. Based on this observation, calculate q for the water and ΔH° for the process, assuming that the heat absorbed by the salt is negligible. CsClO4(s) Cs+(aq) + ClO4- (aq) The specific heat of water is 4.184 J °C-1 g-1. Give the answers in kJ. qH2O = kJ ΔH° = kJ
Assuming that the specific heat of the solution is 4.18
J/(g⋅∘C) and that the calorimeter itself absorbs a negligible
amount of heat, calculate ΔH in kilojoules for the reaction.
Part A Assuming that the specific heat of the solution is 4.18 J/(g . C) and that the calorimeter itself absorbs a negligible amount of heat, calculate AH in kilojoules for the reaction K2O(8)+H20()-2KOH(aq) ανα ΑΣφ ? ΔΗ - kJ Request Answer Submit Provide Feedback Next> Constants Periodic Tab When 1.045...
8 4 points When a 0.456 g sample of salt is dissolved into water in a completely insulated calorimeter (a simple styrofoam coffee cupl. the temperature of the 500 ml water decreases by 0.940°C. What is the heat for the system (the salt dissolving)? O 1.79kJ 0 +1.80 kJ O +214) O 0.214 - 1.96 kJ +1.97 Ooo
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