Given that the enthalpy of neutralization for the reaction of HCl (a strong acid) and NaOH (a strong base) is always -55.90 kJ per mole of H2O formed, what is the concentration of a 65 mL sample of HCl if the enthalpy of neutralization for the reaction was found to be -5.38 kJ, assuming no heat is lost to the calorimeter?       0.96 M     1.48 M     1.60 M     0.38 M     4.63 M

When 10.00 grams of cesium bromate is dissolved in 42.0 grams of water initially at a temperature of 25.00 ºC, the temperature of the solution decreases to 16.11 ºC. Calculate ΔHº for the reaction below in kJ/mol.[You may assume that the reaction takes place inside a perfect calorimeter and that the specific heat capacity of the solution formed is the same as for pure water.Calculate ΔHº for the reaction below in kJ/mol.CsBrO3 (s) ➝ Cs+ (aq) + BrO3 – (aq)       ΔHº= ?

After a few minutes on the hot plate some sodium bicarbonate (NaHCO3) begins to decompose into sodium carbonate, CO₂(g) and H₂O(g). Using standard enthalpies of formation, calculate the enthalpy change for this reaction. Use the following data. The standard enthalpy of formation for NaHCO3 is -997 KJ/Mol and sodium carbonate is -468 KJ/Mol.

Section 5.6 You place 0.0750 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCI. The reaction that occurs is: -> Mg (s) + 2 HCI (aq) → H2 (g) + MgCl2 (aq) The temperature of the solution raises from 20.15 °C to 23.29 °C. What is the enthalpy change or the reaction per mole of Mg? Assume that the specific heat capacity of the solution is 4.20 J/g K and the density of the solution is 1.00 g/mL. 412 kJ/mol 428 kJ/mol -412 kJ/mol -428 kJ/mol

Cold packs are made from ammonium nitrate and water. To measure the enthalpy of this reaction 2.50 grams of NH4NO3 (MW = 80.04 g/mole) is dissolved in enough water to make a 50.0 ml solution in a coffee cup calorimeter of negligible heat capacity.  The temperature decreases from 25.8 C to 21.9 C.  Calculate the molar enthalpy for this reaction.

A 0.602-g sample of isophthalic acid (C8H604) is burned in a bomb calorimeter and the temperature increases from 24.80 °C to 27.05 °C. The calorimeter contains 1.01x10³ g of water and the bomb has a heat capacity of 936 1/°C. The heat capacity of water is 4.1843 g ¹¹. Based on this experiment, calculate AE for the combustion reaction per mole of isophthalic acid burned. 9 kJ/mol

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What is the enthalpy change for the reaction MgO(s) + 2HCl(g) →MgCl2(s) + H2O(l)? Enthalpies of formation are −601.7 kJ/mole for MgO, −92.3 kJ/mole for HCl, −641.6 kJ/mole for MgCl2, and −285.8 kJ/mole for H2O(l).

A calorimeter is calibrated by mixing two aqueous solutions each with a volume equal to 44.4 mL. The reaction is known to produce 1,465 J of heat, and the measured temperature rise is 4.64 K. Heat produced by the reaction is absorbed by the calorimeter and the resulting solution in it. The same calorimeter is used in a subsequent experiment where 44.4 mL of 0.430 mol L-1 HCl are mixed with 44.4 mL of 0.43 of NaOH. The temperature rises by 3.38. Calculate the heat evolved by the reacting system in J *be sure to include the correct sign in your answer*. heat evolved (J) = What is the enthalpy of the neutralization reaction in kJ/mol ? Enthalpy of Reaction (kJ/mol) = kJ/mol

In parts 2, 3 and 4 of this lab, you will be conducting calorimetry experiments on neutralization reactions in solution. Two solutions (each of volume 2.5 mL) will be mixed together to initiate the reaction. What mass of water should be used in the calculation of the heat energy absorbed by the calorimeter? 2.5 g 5.0 g (since the two solutions are mixed together, the volumes and hence their masses are added together).