A reaction of 1.00 gram of NaOH with 100 mL of 1.0 M HCl in a styrofoam calorimeter causes a 10.5°C increase in the temperature of the reaction solution. Assuming the specific heat of the solution is 4.184 J/g°C, density is 1.00 g/mL, and the heat capacity of the styrofoam cup calorimeter is 10.0 JPC, calculate the heat of this reaction per mole of NaOH. ΔΗΞ kJ/mol

A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?

A 32.1 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 25.8°C. Calculate the mass of water in the calorimeter.

In a coffee-cup calorimeter, 120.0 mL of 1.4 M  NaOH  and 120.0 mL of 1.4 M HCL  are mixed. Both solutions were originally at 20.6°C. After the reaction, the final temperature is 30.0°C. Assuming that all the solutions have a density of 1.0  and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCL  by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH =  kJ/mol

When 1.366 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?

25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations. 21.

In a coffee-cup calorimeter, 110.0 mL of 1.3 M and 110.0 mL of 1.3 M are mixed. Both solutions were originally at 22.2°C. After the reaction, the final temperature is 30.9°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH in (kJ/mol). Assume that no heat is lost to the surroundings or to the calorimeter.

The heat of combustion of benzoic acid, HC7H5O2, is 26.38 kJ/g. A 1.640 g sample of benzoic acid is burned in a bomb calorimeter containing 1000.0 mL of water. The temperature of the water increases from 22.25 o C to 27.20 o C. What is the heat capacity of the calorimeter?