1 Experiment 8 Thermochemistry CH 204 Spring 2008 Dr. Brian Anderson Last week Dilutions - Backward and Forward Beer’s Law: A = ecl Determined Molecular Formula for Crystals Thermochemistry The study of heat in chemical reactions. Heat is produced and consumed in chemical reactions in stoichiometric amounts, just like any other reactant or product.2 Thermochem in CH204 We look at two different thermochemical situations: Calorimetry add something hot to something cold heat lost by the hot = heat gained by the cold Hess’s Law Forming chemical bonds releases energy. Breaking chemical bonds requires energy. Add up all the energies to get the heat of reaction, ∆H rxn . Calorimetry Calorimeter – a container that traps heat Put a known mass of water in the calorimeter, add something hot, and measure heat gain by the temperature increase of the water The calorimeter itself also heats up when something hot is added Accounting for heat energy The total amount of heat added is equal to the amount of heat absorbed by the water plus the amount of heat absorbed by the calorimeter: q added = q water + q calorimeter The amount of heat absorbed by the water is equal to the mass of the water times the change in temperature times its specific heat capacity: q water = m w × c w × ∆T C The amount of heat absorbed by the calorimeter is equal to its heat capacity times the change in temperature: q cal = C cal × ∆T C3 Specific heat capacity The amount of heat it takes to raise 1 gram of a substance by 1 degree C Units are J/gK c subscript A word on heat capacities SPECIFIC HEAT CAPACITY is an intensive property. Specific heat capacity tells how much heat (in Joules) is required to raise the temperature of one gram of the substance by one Kelvin. HEAT CAPACITY is an extensive property. It takes into account how much mass you have. Lots o’ Variables! q total = q water + q calorimeter q total = (m C × c s × ∆T C ) + (C cal × ∆T C ) Heat added = –(m H × c H × ∆T H ) Combine ’em all in one equation and you get...4 ...a very useful equation q total = q water + q calorimeter –(m H × c H × ∆T H ) = (m w × c w × ∆T C ) + (C cal × ∆T C ) ∆T = T final – T initial ∆T C = T M – T C (always positive) ∆T H = T M – T H (always negative) This week in lab We will measure the amount of heat given off by 50 ml of hot water, by some chunks of hot metal, and by two chemical reactions Mg + 2H + → Mg 2+ + H 2 + heat MgO + 2H + → Mg 2+ + H 2 O + heat We’ll do all these reactions in a coffee cup calorimeter. The basic operation of calorimetry - Start with a known mass of a solution in the calorimeter. - Drop in something hot, or start a reaction that generates heat. - Close the calorimeter and measure the increase in temperature as heat is generated. - Keep measuring the temperature until it finally levels out.5 Fair warning You will be collecting lots and lots o’ data points, but there are no tables in the lab manual for all this data. All time and temperature data gets recorded directly into the lab notebook. Any loose sheets of data belong to me, and you can start over. Part One: Add hot water to cold 50 mL of cold water (5ºC). Add 50 mL of hot water (75ºC). Final temp should be (75 + 5) ÷ 2 = 40ºC But the final temp will actually be lower than that because the cup itself will absorb a little bit of the heat. Heat Capacity We will use the data in part 1 to calculate the heat capacity of the cup, in units of J/K. This will tell us how many Joules of heat the cup absorbs for every K (or degree C) the cup heats up. –(m H × c H × ∆T H ) = (m w × c w × ∆T C ) + ( C cal × ∆T C )6 Part 2 Unknown Metal We will determine the identity of an unknown metal by calculating its specific heat capacity. –(m M × c M × ∆T H ) = (m C × c s × ∆T C ) + (C cal × ∆T C ) Unknown summary sheet Specific heat capacity of your unknown metal and the identity of your metal. Observations are valid data. What does your metal look like? Is it magnetic? What is its density? Parts 3 and 4 The reactions of magnesium and magnesium oxide with HCl. Mix these continuously, especially the MgO. IMPORTANT: Use 2.0M HCl to react with the Mg metal (Part 3). Use 6.0M HCl to react with the MgO (Part 4). HCl in the hood is 6.0 M.7 Parts 3 and 4 Calculate how much heat is given off by the reaction: –heat added = (m s × c s × ∆T C ) + (C cal × ∆T C ) Divide the heat added by the moles of Mg or MgO used to get ∆H in J/mole Making graphs in Excel You’ll have a total of 5 graphs (2 for Part 1, and 1 each for parts 2, 3, and 4). You will use the graphs to determine ∆T C . You can draw lines on the graphs yourself or have Excel do it for you. Get it right the first time 1) Start recording temps before starting the reaction 2) Cover and swirl immediately! 3) Continue recording temps on the same timeline throughout the experiment. 4) Keep taking temperature readings until the temp is constant or declining8 Working with a partner Put your partner’s name on everything, but turn in your own report, with your own graphs and your own unknown summary sheet. Some Fatherly Advice Start the report early Don’t wait until all the TA office hours have passed before you start on this. The calculations are not hard, but students have more questions on this lab report than on any other.9 The Post-Lab One calculation of specific heat capacity. Two calorimetry problems. Two Hess’s Law problems. No partial credit this time! There is a hint sheet on the Freebies page. Everybody get a 10 on this! Next Week’s Quiz • Know the calorimetry equation • Be able to do Hess’s Law problems • Know the definitions of the terms we’re using this week: heat capacity, specific heat capacity, enthalpy of formation, standard state, Hess’s