What is the heat of a reaction, in joules, with a total reaction mixture volume of 67.3 mL if the reaction causes a temperature change of 5.9 °C in a calorimeter? Assume that the reaction mixture has a density of 1.00 g/mL and a specific heat of 4.184 J/g-°C. The calorimeter has a heat capacity of 10.0 J/°C.

100.0 ml of 0.115 m potassium hydroxide solution is mixed with 75.0 ml of 0.245 M nitric acid solution in a coffee cup calorimeter. Before mixing, both solutions are initially at 23.85 C;after mixing, the temperature of the mixture in the coffee cup calorimeter increases to 26.30 C. Determine the enthalpy change(delta h) of reaction in kJ/mol for the reaction as written below. KOH(aq) + HNO3(aq) ⮕ KNO3(aq) + H2O(aq) Assume the  resulting  solution density is 1.03 g/mL. Specific heat of solution=4.20 J/g C

When 1.836 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?

When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ