When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jgl°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? O a. -83.2 kJ b. -73.6 kJ C. -76.0 kJ O d. -80.8 kJ O e. -78.4 kJ

In a Calorimetry experiment, a chemical reaction causes the temperature of the solution in the chamber to raise from 20.1 °C to 69.3 °C. Knowing that the solution weights 600. g, and specific heat of the solution is 4.18 J g–1 K–1, the heat released by the reaction is ______ .

When 15.0 mL of 3.00 M NaOH was mixed in a calorimeter with 12.5 mL of 3.00 M HCl, both initially at room temperature (22.0 °C), the temperature increased to 29.0 °C. The resultant salt solution had a mass of 27.50 g and a specific heat capacity of 3.74 J K-1 g-1. What is the heat capacity of the calorimeter (in J/°C)? Note: the molar enthalpy of neutralization per mol is -55.84 kJ mol-1

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