In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCI are mixed. Both solutions were originally at 24.0°C. After the reaction, the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C g, calculate the enthalpy change for the neutralization of HCI by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ- kJ/mol

A student conducts a calorimetry experiment on an unknown metal object. The unknown metal object with a mass of 82.522 g is heated to 100.5 °C and then transferred to a coffee-cup calorimeter containing 67.225 g of water at 22.3 °C. If the metal object and the water reach a final temperature of 30.5 °C and the heat absorbed by the water was calculated to be 2310 J. What is the specific heat of this metal object? (The specific heat of water is 4.18 J/g°C)

A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What is the total heat for the dissolution reaction of the 5.71 g of salt?

A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Given that 154.81 g of solution increased in temperature by 4.82 °C, how much heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g･°C     ______ J?

If 0.066 mol of hydrochloric acid (HCl) is mixed with 0.066 mol of sodium hydroxide (NaOH) in a "coffee cup" calorimeter, the temperature of 5.0 g of the resulting solution increases from 25.0°C to 30.0°C.  Given that the energy released is 1.2 × 101 cal when the specific heat of the resulting solution is 1.00 cal/g−°C, use a conversion factor to convert the energy released to joules (J).  Enter your answer in scientific notation. Be sure to answer all parts.

A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 38.86°C. The specific heat capacity of water is 4.184 J g.°C and the density of water is g 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = = °C

In an experiment, 30.0 g of metal was heated to 98.0°C and then quickly transferred to 50.0 g of water in a calorimeter. The heat capacity of the calorimeter with the water was 211 J/°C. The initial temperature of the calorimeter was 27.0°C, and the final temperature after addition of the metal was 32.5°C. What is the value of the specific heat capacity of the metal?

When 1.416 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?

1 Cal= 4.18 kJ

In an experiment, 28.0 g of metal was heated to 98.0°C and then quickly transferred to 150.0 g of water in a calorimeter. The initial temperature of the water was 24.5°C, and the final temperature after the addition of the metal was 32.5°C. Assume the calorimeter behaves ideally and does not absorb or release heat.  What is the value of the specific heat capacity (in J/g•°C) of the metal?