All of the heat from the combustion of 39.10 mL of C,H, is transferred to 5.175 L of water at 26.9°C. What will the final temperature of the water be, in °C? (The density of C_H() is o.8765 g/mL. Assume the density of water is 1.00 g/mL and its specific heat is 4.184 J/(g °C).)

The combustion of 1.00 mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.83 g of glucose is burned in a calorimeter containing 773 g of water, and the temperature of the assembly increases from 20.10 °C to 24.56 °C, what is the heat of the calorimeter in kJ/°C MW of glucose is 180 g/mol?

[References] In a coffee-cup calorimeter, 100.0 mL of 1.3 M NaOH and 100.0 mL of 1.3 M HCl are mixed. Both solutions were originally at 24.3°C. After the reaction, the final temperature is 33.0°C. Assuming that all the solutions have a density of 1.0 g/cm³ 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. kJ/mol AH = Submit Answer Try Another Version 1 item attempt remaining 4 C C A 6 T

Titanium reacts with iodine to form titanium(III) iodide, emitting heat:2 Ti(s) + 3 I2(g) ---------> 2 TiI3(s) ∆H°rxn = -839 kJDetermine the masses of titanium and iodine that react if 1.55 x 103 kJ of heat is emitted by the reaction.