<p> Leader: Kia Birnbaum Hess’s Law and Enthalpy Course: CHEM177 Supplemental Instruction Instructor: Anand Iowa State University Date: March 3rd, 2017</p><p>Concept Check 1. Fill in the blank a. A _____ function means that the value is independent of the pathway.</p><p> b. A calorimeter at constant pressure is known as a ______calorimeter.</p><p> c. A calorimeter at constant volume is known as a ______calorimeter.</p><p> d. Breaking bonds ______energy.</p><p> e. Standard Enthalpy of Formation is the heat evolved from the formation of ______of product from its constitute elements in their ______form. </p><p>Practice Problems 2. Determine the enthalpy of reaction for CH3COCH3(l) + 2 O2(g)  CH3COOH(l) + CO2(g) + H2O(g) Using Hess’s law of constant heat summation and given: CH3COCH3(l) + 4 O2(g)  3 CO2(g) + 3 H2O(l) ΔH= -1787.0 kJ H2O(l)  H2O(g) ΔH= -44.1 kJ CH3COOH(l) +2 O2(g)  2 CO2(g) + 2 H2O(l) ΔH= -835 kJ</p><p>3. Calculate the standard enthalpy of formation of ozone [ΔH°f(O3)] from the following information: For the reaction, Pb(s) + C(s) + O3(g)  PbCO3(s) the enthalpy of reaction (ΔHrxn) is -841.0 kJ and the standard enthalpy of formation for PbCO3(s) is -699.0 kJ/mol. </p><p>1060 Hixson-Lied Student Success Center v 515-294-6624 v [email protected] v http://www.si.iastate.edu 4. Meals-ready-to-eat (MREs) are military meals that can be heated on a flameless heater. The heat is produced by the following reaction: Mg(s) + 2 H2O(l)  Mg(OH)2(s) + 2 H2(g) a. Calculate the standard enthalpy change for this reaction. (ΔH°f(H2O(l))= -285.83 kJ/mol, ΔH°f(Mg(OH)2(s))= -924.7 kJ)</p><p> b. Calculate the number of grams of Mg (mm=24.21 g) needed for this reaction to release enough energy to increase the temperature of 75 mL of water from 21 to 79°C.</p><p>5. 5.00 kg of a hot metal at 200.0 deg C is added to 25.0 kg of water at 30.0 deg C. What is the final temperature of the metal? The specific heat of the metal is 0.800 J/g*deg C and for water it is 4.184 J/g*deg C. </p><p>Challenge Question 3 6. Ammonia (NH3) boils at -33°C; at this temperature it has a density of 0.81 g/cm . The enthalpy of formation of NH3(g) is -46.2 kJ/mol, and the enthalpy of vaporization of NH3(l) is 23.2 kJ/mol. Calculate the enthalpy change when 1 L of liquid NH3 is burned in air to give N2(g) and H2O(g). </p>