When a 2.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 1.25 kJ⋅K−1, the temperature decreases by 0.400 K. Calculate the molar heat of solution of KSCN.

A quantity of 85.0 mL of 0.600 M HCl is mixed with 85.0 mL of 0.600 M KOH in a constant-pressure  calorimeter. The initial temperature of both solutions is  the same at 17.35°C, and the final temperature of the  mixed solution is 19.02°C. What is the heat capacity of  the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is −56.2 kJ/mol.

A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC.  After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams.  For this problem, assume the  specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures.  What is the heat transferred by this reaction, in Joules?

100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?

A change in a system occurs such that 31.1 J of work is done by the surroundings and 22.4 J of heat flows from the system to the surroundings. What is the change in internal energy of the system?

When a 7.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 5.28 kJ⋅K^-1, the temperature decreases by 0.330 K Calculate the molar heat of solution of KSCN.

When a 6.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 3.74 kJ · K¯¹, the temperature decreases by 0.400 K. Calculate the molar heat of solution of KSCN. ΔΗsoln = kJ/mol

A quantity of 100.0 mL of 1.0 M HCl and 100.0 mL of 1.0 M NaOH are mixed in a calorimeter. The initial temperatures of the HCl and NaOH solutions are the same at 20.0°C and the final temperature of the mixture is 27.0oC.  Calculate the heat of neutralization for the reaction in kJ/mole of NaOH.  Assume the density and specific heat of the solutions are the same as pure water and that no heat was lost to the surroundings.

Consider the change in the internal energy of a system. what is the change in the internal energy, in joules, of a system that does 4.75 x 10^5 J of work, while 3.05 x 10^6J of heat is transferred into the system and 8.25 x 10^6J of heat is transferred from the system to the environment?