Enthalpy, Hess Cycles and Calorimetry PDF

Chemical Energetics 1 THERMODYNAMICS First Law Energy can be neither created nor destroyed but...

Chemical Energetics 1 THERMODYNAMICS First Law Energy can be neither created nor destroyed but it can be converted from one form to another. all chemical reactions are accompanied by some form of energy change changes can be very obvious (gas burning) but in many cases it goes unnoticed Enthalpy a measure of the heat content of a substance at constant pressure you cannot measure the actual enthalpy of a substance you can measure an ENTHALPY CHANGE at CONSTANT PRESSURE written as the symbol ∆Η , “delta H ” Enthalpy change (∆Η) = Enthalpy of products - Enthalpy of reactants EXOTHERMIC REACTION ENDOTHERMIC REACTION E E N N T T H H A Ea A Ea L P L P Y Y reactants products Knockhardy Publishing H H products reactants Enthalpy of reactants > products Enthalpy of reactants < products ∆Η = - ive ∆Η = + ive EXOTHERMIC Heat given out ENDOTHERMIC Heat absorbed Examples EXOTHERMIC combustion of fuels CH4 + 2O2 —> CO2 + 2H2O respiration C6H12O6 + 6O2 —> 6CO2 + 6H2O (oxidation of carbohydrates such as glucose) ENDOTHERMIC photosynthesis 6CO2 + 6H2O —> C6H12O6 + 6O2 thermal decomposition CaCO3 —> CaO + CO2 of calcium carbonate © KNOCKHARDY PUBLISHING 2015 2 Chemical Energetics Standard Enthalpy Changes enthalpy values vary with the conditions - so standard conditions are needed a substance will then be in its standard state... Pressure:- 100 kPa (1 atm) A stated temperature:- usually 298K (25°C) as a guide, just think of a substance under normal laboratory conditions assign the correct subscript [ e.g. (g), (l) or (s) ] to indicate which state it is in any solutions are of concentration 1 mol dm-3 to tell if standard conditions are used we modify the symbol for ∆Η. Enthalpy Change Standard Enthalpy Change (at 298K) ∆Η ∆Η 298 Enthalpy Change of Reaction ( ∆Ηr or ∆rΗ) (NO sign) Definition The enthalpy change associated with a stated reaction. Knockhardy Publishing Enthalpy Change of Combustion ( ∆Ηc or ∆cΗ) (NO sign) Definition The enthalpy change when ONE MOLE of a substance undergoes complete combustion Standard Enthalpy Change of Combustion ( ∆Η°c ) (there is a sign) Definition The enthalpy change when ONE MOLE of a substance undergoes complete combustion under standard conditions. All reactants and products are in their standard states. Values Always exothermic Example(s) C(graphite) + O2(g) ——> CO2(g) C2H5OH(l) + 3O2(g) ——> 2CO2(g) + 3H2O(l) Notes To aid balancing the equation, remember that you get one carbon dioxide molecule for every carbon atom in the original molecule and a water molecule for every two hydrogen atoms. Having done this, go back and balance the oxygen. Q.1 Write equations representing the (standard) enthalpy change of combustion of... methane methanol cyclohexane hydrogen carbon © KNOCKHARDY PUBLISHING 2015  Chemical Energetics 3 Enthalpy Change of Formation ( ∆Ηf or ∆f Η) Definition The enthalpy change when ONE MOLE of a compound is formed from its elements. Standard Enthalpy Change of Formation ( ∆Η°f) (there is a sign) Definition The enthalpy change when ONE MOLE of a substance is formed in its standard state from its elements in their standard states. Values Usually, but not exclusively, exothermic Example(s) 2C(graphite) + ½O2(g) + 3H2(g) ——> C2H5OH(l) Notes elements In their standard states have zero enthalpy of formation carbon is usually taken as the graphite allotrope. Q.2 Construct equations representing the standard enthalpy change of formation of methane sulphuric acid sodium chloride water carbon dioxide Knockhardy Publishing Q.3 What do you notice about the equations for... the standard enthalpy change of combustion of hydrogen and the standard enthalpy change of formation of water? the standard enthalpy change of combustion of carbon and the standard enthalpy change of formation of carbon dioxide? Enthalpy of Neutralisation ( ∆Ηneut or ∆neut Η) Definition Enthalpy change when ONE MOLE of water is formed from its ions in dilute soln. Values Exothermic Equation H+(aq) + OH¯(aq) ——> H2O(l) Notes A value of -57kJ mol-1 is obtained when strong acids react with strong alkalis. © KNOCKHARDY PUBLISHING 2015 4 Chemical Energetics Bond Dissociation Enthalpy (Energy) Definition Energy required to break ONE MOLE of gaseous bonds to form gaseous atoms. Values Endothermic Energy must be put in to break any chemical bond Example Cl2(g) ——> 2Cl(g) Notes the strength of a bond depends on its environment so MEAN values are quoted making a bond is an exothermic process as it is the opposite of breaking a bond for diatomic gases, the bond enthalpy is twice the enthalpy of atomisation the smaller the bond enthalpy, the weaker the bond and the easier it is to break Some mean bond enthalpies (in kJ mol-1) (values may differ slightly in other texts) H-H 436 H-F 562 N-N 163 C-C 346 H-Cl 431 N=N 409 C=C 611 H-Br 366 N≡N 944 C≡C 837 H-I 299 P-P 172 C-O 360 H-N 388 F-F 158 C=O 743 H-O 463 Cl-Cl 242 Knockhardy Publishing C-H 413 H-S 338 Br-Br 193 C-N 305 H-Si 318 I-I 151 C-F 484 P-H 322 S-S 264 C-Cl 338 O-O 146 Si-S 176 C-Br 276 O=O 496 Si-O 374 HESS’S LAW “The enthalpy change is independent of the path taken” ∆Ηr A B ∆Η1 ∆Η3 ∆Η2 X Y ∆Ηr = ∆Η1 + ∆Η2 + ∆Η3 applying Hess’s Law enables one to calculate enthalpy changes from other data used for calculating changes which can’t be measured directly - Lattice Enthalpy used for calculating - enthalpy change of reaction from bond enthalpy - enthalpy change of reaction from ∆Η°c - enthalpy change of formation from ∆Η°f © KNOCKHARDY PUBLISHING 2015  Chemical Energetics 5 Enthalpy change of reaction from average bond enthalpies Theory Imagine that, during a reaction, all the bonds of reacting species are broken and the individual atoms join up again but in the form of products. The overall energy change will depend on the difference between the energy required to break the bonds and that released as bonds are made. energy released making bonds > energy used to break bonds... EXOTHERMIC energy used to break bonds > energy released making bonds... ENDOTHERMIC Example Calculate the enthalpy change for the hydrogenation of ethene H H ∆Η1 H H C C + H H H C C H H H H H Breaking bonds - ∆Η2 ∆Η3 Breaking bonds - ENDOTHERMIC ENDOTHERMIC H H H H C C H H Knockhardy Publishing ∆Η2 1 x C = C bond @ 611 = 611 4 x C H bonds @ 413 = 1652 1 x H H bond @ 436 = 436 Total energy required to BREAK bonds of reactants = 2699 kJ mol -1 ∆Η3 1 x C 6 x C C bond @ 346 = 346 H bonds @ 413 = 2478 -1 Total energy required to BREAK bonds of products = 2824 kJ mol Applying HESS'S LAW ∆Η1 = ∆Η2 - ∆Η3 = 2699 - 2824 = -125kJ Q.4 Using the average bond enthalpies in your notes, calculate the standard enthalpy changes of reaction for the following reactions. a) H2(g) + ½O2(g) ——> H2O(g) b) CH4(g) + 2O2(g) ——> CO2(g) + 2H2O(g) c) H2(g) + Cl2(g) ——> 2HCl(g) d) C2H5OH(g) + HBr(g) ——> C2H5Br(g) + H2O(g) © KNOCKHARDY PUBLISHING 2015 6 Chemical Energetics Enthalpy change of reaction from enthalpy changes of combustion and formation Formation If you formed the products from their elements you should need the same amounts of every substance as if you formed the reactants from their elements. By applying Hess’s Law... ELEMENTS ∆Ηr ∆Η f A B ∆Η f ∆Ηf ∆Ηf REACTANTS ∆Ηr ELEMENTS PRODUCTS Knockhardy Publishing ∆Ηr = Σ ∆Η f (PRODUCTS) Σ ∆Η f (REACTANTS) example Calculate the standard enthalpy change for the following reaction, given that the standard enthalpies of formation of water, nitrogen dioxide and nitric acid are -286, +33 and -173 kJ mol-1 respectively. [oxygen’s value is ZERO as it is an element ] 2H2O(l) + 4NO2(g) + O2(g) ——> 4HNO3(l) applying Hess’s Law... ∆Η°r = [ 4(-173) ] - [ 2(-286) + 4(+33) + 0 ] = -252 kJ Q.5 If the standard enthalpy changes of formation of SO2(g) and SO3(g) are -296 and -395 kJ mol-1 respectively, calculate the enthalpy change of reaction of... 2SO2(g) + O2(g) ——> 2SO3(g) © KNOCKHARDY PUBLISHING 2015  Chemical Energetics 7 Combustion If you burned all the products you should get the same amounts of CO2 and H2O etc. as if you burned the reactants. Applying Hess’s Law... REACTANTS DH r ∆Ηr A B DHc PRODUCTS ∆Ηc ∆Ηc DHc OXIDATION OXIDATION PRODUCTS PRODUCTS ∆Ηr = Σ ∆Η c (REACTANTS) Σ ∆Η c (PRODUCTS) Knockhardy Publishing example Calculate the standard enthalpy change of formation of methane, given that the standard enthalpies of combustion of carbon, hydrogen and methane are -394, -286 and -890 kJ mol-1 respectively. C(graphite) + 2H2(g) ——> CH4(g) applying Hess’s law... ∆Η°r = [ (-394) + 2(-286) ] - [ (-890) ] = -74 kJ mol-1 Q.6 Calculate the enthalpy change of reaction for H2 + C2H4 ——> C2H6 given that the enthalpy changes of combustion of H2, C2H4 and C2H6 are -286, -1409 and -1560 kJ mol-1 respectively. Compare this value with that obtained using average bond enthalpies. © KNOCKHARDY PUBLISHING 2015 8 Chemical Energetics Measuring Enthalpy Changes Calorimetry involves the practical determination of enthalpy changes usually involves heating (or cooling) known amounts of water water is heated up reaction is EXOTHERMIC water cools down reaction is ENDOTHERMIC Calculation The energy required to change the temperature of a substance can be found; q = m x c x ∆Τ where q = heat energy kJ m = mass kg c = Specific Heat Capacity kJ K -1 kg -1 [ water is 4.18 ] ∆Τ = change in temperature K ∆Τ The value of ∆Τ is usually calculated graphically by measuring the temperature Knockhardy Publishing changes before, during and after a reaction. Graphical method ★ ★ ★ ★ The temperature is taken every half ★ ★ ★ ★ ★ ★ ★ minute before mixing the reactants. Temperature / °C Reactants are mixed after 3 minutes. ∆Τ Further readings are taken every half minute as the reaction mixture cools. Extrapolate the lines as shown and calculate the value of ∆Τ. ★ ★ ★ ★ ★ 1 3 5 7 9 Time / minutes Example 1 When 0.18g of hexane underwent complete combustion, it raised the temperature of 100g (0.1kg) water from 22°C to 47°C. Calculate its enthalpy of combustion. Heat absorbed by the water (q) = 0.1 x 4.18 x 25 = 10.45 kJ Moles of hexane burned = mass / Mr = 0.18 / 86 = 0.00209 Enthalpy change = heat energy / moles = − 10.45 / 0.00209 ANS − 5000 kJ mol -1 © KNOCKHARDY PUBLISHING 2015  Chemical Energetics 9 Example 2 25cm3 of 2.0M HCl was added to 25cm3 of 2.0M NaOH in an insulated beaker. The initial temperature of both solutions was 20°C. The reaction mixture was stirred to ensure mixing and the highest temperature reached by the solution was 33°C. Calculate the Molar Enthalpy of Neutralisation. Temperature rise (∆Τ) = 306K - 293K = 13K Volume of resulting solution = 50cm3 = 0.05 dm3 Equivalent mass of water = 50g = 0.05 kg Heat absorbed by the water (q) = 0.05 x 4.18 x 13 = 2.717 kJ Moles of HCl reacting = 2 x 25/1000 = 0.05 mol Moles of NaOH reacting = 2 x 25/1000 = 0.05 mol Equation NaOH + HCl ——> NaCl + H2O Moles of water produced = 0.05 mol Enthalpy change per mol (∆Η) = − ( heat energy / moles of water ) = − 2.717 / 0.05 ANS − 54.34 kJ mol -1 Knockhardy Publishing Q.7 What is the usual value for the Molar Enthalpy of Neutralisation ? Why might the value calculated from the reaction between sodium hydroxide and ethanoic acid differ from the usual value? Results from simple calorimetry experiments are seldom very accurate. Make a list of possible sources of error and suggests improvements to the experiment. © KNOCKHARDY PUBLISHING 2015 10 Chemical Energetics Enthalpy of Combustion of Alkanes 1. Write the equation representing the Standard Enthalpy Change of Combustion of heptane, C7H16............................................................................................................................................... 2. Using the data, plot a graph of Enthalpy of Combustion against number of carbon atoms. Compound Enthalpy of Combustion / kJ mol-1 CH4 - 890 C2H6 - 1560 C3H8 - 2220 C4H10 - 2877 C5H12 - 3509 C6H14 - 4194 C8H18 - 5512 3. Use your graph to calculate the following Knockhardy Publishing a) the value of the Enthalpy Change of Combustion of heptane.......................... b) an approximate value for the Enthalpy Change of Combustion of hydrogen.......................... 4. State, giving reasons, any advantages of using butane as a household fuel...................................................................................................................................................................................................................................................................................................................................................................................................................................................................... 5. State, giving reasons, any disadvantages of using butane as a household fuel...................................................................................................................................................................................................................................................................................................................................................................................................................................................................... 6. Calculate the amount of heat produced when 1kg of the following undergo complete combustion. a) CH4 b) C4H10 © KNOCKHARDY PUBLISHING 2015