A 3.50 g sample of KOH (at 22.3 °C) is dissolved in a 5.50 M HCl solution in a coffee cup calorimeter. The total volume of the resulting solution is 250 mL and its temperature rises from the initial value of 22.3 °C (before KOH addition) to 37.8 °C. Calculate ΔH (in kJ/mol) of the dissolution and neutralization of KOH.
Assume that the density of the solution is 1.00 g/mL and that the specific heat of the solution is the same as that for water, 4.184 J/(g·K).
A.) −10.8 kJ/mol
B.)+104.7 kJ/mol
C.) −259.6 kJ/mol
D.) −16.2 kJ/mol
E.) +16.2 kJ/mol
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When 27.0 mL of 0.500 M H2SO4 is added to 27.0 mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate ΔH of this reaction. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.) Answer: ______ kJ/mol H2O
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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 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 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
When 22.00 mL of 0.5000 M H_2SO_4 is added to 22.00 mL of 1.000 M kOH in a coffee-cup calorimeter at 23.50 degree C, the temperature rises to 30.17 degree C. Calculate delta H of this reaction. (Assume that the total volume is the sum of the individual assumes and that the density and specific heat capacity of the solution are the same for pure water.) (d for water = 1.00 g/mL; c for water - 4.184 J/g degree C.)...
When 16.3 g KOH is dissolved in 94.3 g of water in a coffee-cup calorimeter, the temperature rises from 18.9 °C to 30.16 °C. What is the enthalpy change per gram (in J/g) of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g×K. Water has a density of 1.00 g/ml. Be sure to enter the correct sign (+/-). Enter to 1 decimal place.
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