When a 6.00 g sample of KCl is dissolved in water in a calorimeter that has a total heat capacity of 3.96 kJ⋅K−1, the temperature decreases by 0.350 K. Calculate the molar heat of solution of KCl.

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. What is the total mass inside the calorimeter in grams? What is the change in temperature, in °C inside the calorimeter ?

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?

When a 6.00 g sample of KBr is dissolved in water in a calorimeter that has a total heat capacity of 3.58 kJ - K¯¹, the temperature decreases by 0.280 K. Calculate the molar heat of solution of KBr. AH soln = I kJ/mol

A 50.0-g sample of a copper-zinc alloy is heated to 100.0oC. The hot metal is quickly added to 100.0 g of water in a Styrofoam cup calorimeter. The initial temperature of the water is 25.00oC and the specific heat of water is 4.184 J·g–1·K–1. If the final temperature of water and alloy is 28.30oC, what is the specific heat of alloy in J·g–1·K–1?           (A) 0.276          (B) 0.385          (C) 0.697          (D) 2.09

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.

You add some of the white crystals to a small test tube filled with water. The water in the test tube was initially at room temperature (25˚C). Once the crystals were added and the tube was stirred, the temperature of the solution decreased to about 15˚C and all of the crystals dissolved. what is the change in enthalpy (∆H) for this process?

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.85 kg sample of C,H,,S from -0.2 °C to 10.8 °C. The experiment shows that 4.04 × 10" J of heat are needed. What can the chemist report for the molar heat capacity of C,H,S? Round your answer to 3 12 significant digits. |J•mol 1 ·K x10 ?

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

A chemist dissolved an 10.8-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 23.9°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. %3D =Db Calculate the heat of solution for KOH in kJ/mol. kJ/mol heat of solution =