# 5184) kJ/mol in Visual C#.NET Recognize Data Matrix ECC200 in Visual C#.NET 5184) kJ/mol

5184) kJ/mol
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Grxn = 2(5184) [2(8671) + 0000] = 6974 kJ/mol = Grxn + RT ln Q
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(100)2 = ( 69 74 kJ)(1000 J/kJ) + 8314 J (500 K )ln ( 2 00)2 (0 500) mol K = 7 262 10 4 J/mol Note that Q, when at equilibrium, becomes K This equation gives us a way to calculate the equilibrium constant, K, from a knowledge of the standard Gibbs free energy of the reaction and the temperature If the system is at equilibrium, then G = 0 and the equation above becomes: G = RT ln K = 2303 RT log K For example, calculate G for: 2 O3 ( g ) 3O2 ( g ) K p = 4 17 1014
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Note: = 298 K Answer: G = RT ln K (8314 J) = ( 298K )ln 4 17 1014 ( molK) = 8 3 4 10 4 J/mol
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The most common thermodynamic experiment is a calorimetry experiment such as experiment 13 in Experimental chapter In this experiment the heat of transition or heat of reaction is determined The experiment will require a balance to determine the mass of a sample and possibly a pipet to measure a volume, from which a mass may be calculated using the density A calorimeter, usually a polystyrene (Styrofoam) cup, is needed to contain the reaction Finally, a thermometer is required Tables of heat capacities or specific heats may be provided Mass and possible volume measurements, along with the initial and final temperatures, are needed Remember: you measure the initial and final temperature so you can calculate the change in temperature After the temperature change is calculated, there are several ways to proceed If the calorimeter contains water, the heat may be calculated by multiplying the specific heat of water by the mass of water by the temperature change The heat capacity of the calorimeter may be calculated by dividing the heat by the temperature change If a reaction is carried out in the same calorimeter, the heat from that reaction is the difference between the heat with and without a reaction Do not forget, if the temperature increases, the process is exothermic and the heat has a negative sign The opposite is true if the temperature drops
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