Macmillan Learning Revell SECOND EDITION q= A chemist dissolved an 12.7-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 27.6 °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. Calculate the heat of solution for KOH in kJ/mol. Macmillan Learning heat of solution = kJ kJ/mol

A 6.55 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?

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

In a coffee-cup calorimeter, 100.0 mL of 1.1 M    NaOH and 100.0 mL of 1.1 M   HCI are mixed. Both solutions were originally at 22.8°C. After the reaction, the final temperature is 30.2°C. Assuming that all the solutions have a density of 1.0 g/cm^3 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. ΔH = ---------  kJ/mol