Given the following information, calculate the heat of solution for the salt in the unit of kJ. A calorimeter contains 44.96 g of water. The temperatures of the calorimeter and water are both 22.6 degrees Celsius. 2.42 g of salt is dissolved in the water. Then, the temperature falls to (2.2x10^1) degrees Celsius. (Note: the heat capacity of this calorimeter is 30.1 J/degree Celsius. Pay attention to the sig. figs. in your calculation.)

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.61 kg sample of a pure substance from 3.0 °C to 24.2 °C. The experiment shows that 32. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. 1 - 1 ·K x10

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

In a coffee-cup calorimeter, 59.0 mL of 0.100 M AgNO3 and 59.0 mL of 0.100 M HCI are mixed to yield the following reaction. Ag (aq) + Cl(aq) → AgCl(s) The two solutions were initially at 19.10°C, and the final temperature is 19.90°C. Calculate the heat that accompanies this reaction in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 118.0 g and has a specific heat capacity of 4.18 1/°C 9- 407 kJ/mol

A chemist dissolved an 14.2-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 30.5 ∘C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g⋅°C. ?=   kJ Calculate the heat of solution for KOH in kJ/mol.

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains  8.80kg  of water at  20.5°C . During the reaction  66.3kJ  of heat flows out of the flask and into the bath. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is  4.18·J·g−1K−1 . Be sure your answer has the correct number of significant digits.   °C

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.   If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt?   How many moles of the unknown salt were used in the reaction ?     _______ J?

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.50kg of water at 38.9°C. During the reaction 83.3kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18J·g−1·K−1. Be sure your answer has the correct number of significant digits.

A 42.0 g sample of water at 100.00°C was placed in an insulated cup. Then 15.4 g of zinc metal at 23.60°C was added to the water. The temperature of the water dropped to 97.52°C. What is the specific heat of zinc? Assume the specific heat is that of pure water, 4.18 J/(g⋅°C).

A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains  9.80kg  of water at  34.0°C . During the reaction  139.kJ  of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is  4.18·J·g−1K−1 . Be sure your answer has the correct number of significant digits. °C