A chemist dissolve a 13.4 g sample of KOH in 115.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 23.8 °C. How much heat energy was required to dissolve the sample of KOH? Calculate the heat of solution in kJ/mol. Assume the specific heat of the solution is 4.184 J/g ·°C. please help with work shown. sci notation and correct sig figs as well
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A chemist dissolve a 13.4 g sample of KOH in 115.0 grams of water in a...
When a 8.8-g sample of NaBr was combined with 105 grams of water in a coffee cup calorimeter, the water temperature decreased by 6.57 °C. Assume the specific heat of solution is 4.184 J/g.°С. Find the heat lost by water in J. Calculate the heat of solution for NaBr in kJ/mole. Heat lost by water? Heat of solution?
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...
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.
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
Calculate the enthalpy (in kJ) per mole of KOH when 3.25 g KOH is added to H2SO4 in a coffee cup calorimeter to make 123.2 mL of total solution with density 1.06 g/mL. Assume the specific heat capacity of the solution is 4.184 J/g°C, that no heat is lost to the surroundings and that the final temperature of the solution is 7.52°C higher than the starting temperature.
4. 4.21 g of KOH is mixed with 150.00 g of water at 25.3°C in a coffee cup calorimeter. The temperature rises to a maximum of 31.2 °C. Calculate the molar heat of solution of KOH. The heat capacity of the calorimeter is 92.7J/°C. Take the specific heat of the KOH solution to be 3.90 J/gºC.
When a 5.12-g sample of solid sodium nitrate dissolves in 31.1 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 25.00 oC to 16.37 oC. Calculate H in kJ/mol NaNO3 for the solution process. NaNO3(s) Na+(aq) + NO3-(aq) The specific heat of water is 4.18 J/g-K. We were unable to transcribe this imageWe were unable to transcribe this imagethermometer stirrer coffee cups containing reaction mixture When a 5.12-g sample of solid sodium nitrate dissolves in...
When a 9.55 g sample of solid NaOH dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 23.6C to 47 for the solution process. (Assume that the specific heat of the solution is the same as that of pure water.) . .4 °C. Calculate AH (in kJ/mol NaOH)