When a 3.00-g sample of KCl was added to 3.00 × 102 g of water
in a coffee cup calorimeter, the
temperature decreased by 1.05 °C. How much heat is involved in the
dissolution of the KCl?
please show work thank you
When a 3.00-g sample of KCl was added to 3.00 × 102 g of water in...
A 0.400 g sample of KCl(s) is added to 50.0 g of water in a calorimeter. If the temperature decreases by 0.95˚C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g˚C?
A 0.400 g sample of KCl(s) is added to 50.0 g of water in a calorimeter. If the temperature decreases by 0.95˚C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g˚C?
When a 7.82-g sample of solid potassium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 22.7 °C to 59.2 °C. What is ΔH for the dissolution of KOH in water, as shown below? KOH(s) → K+(aq) + OH−(aq) Assume that all solutions have the same specific heat as water.
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 .500g sample of KCL is added to 50g of water initially at 25 degrees celsius in a calorimeter. The final temperature of the solution is 23.95 degrees celsius. What is the heat involved per mol of KCL?
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.
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
When 1.00 g of CaCl2 is added to 50.0 g of water in a coffee-cup calorimeter, it dissolves according to the following eqn: CaCl2 (s) Ca2 (aq) + 2Cl (aq) The temperature of the solution rises from 25.00°C to 28.51 °C. Assuming that all the heat flow involved in the reaction is transferred to the water, calculate q Also, assume that the csoln is equal to cwater Which is 4.18 J/g °C
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.