5184) kJ/mol in Visual C#.NET

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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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Thermodynamics 131
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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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1 Be sure your units cancel giving you the unit desired in the final answer 2 Check your significant figures 3 Don t mix energy units, joules, and calories 4 Watch your signs in all the thermodynamic calculations They are extremely important 5 Don t confuse enthalpy, H, and entropy, S 6 Pay close attention to the state of matter for your reactants and products, and choose the corresponding value for use in your calculated entropies and enthalpies 7 Remember: products minus reactants 8 Hf and Gf are for 1 mol of substance Use appropriate multipliers if needed 9 Gf and Hf for an element in its standard state are zero 10 All temperatures are in kelvin 11 When using G = H rxn T S rxn, pay particular attention to your enthalpy and entropy units Commonly, enthalpies will use kJ and entropies J
132 U Step 4 Review the Knowledge You Need to Score High
U Review Questions
Answer the following questions You have 20 minutes You may not use a calculator You may use the periodic table at the back of the book Choose the type of energy that best relates to questions 1 4 (A) (B) (C) (D) (E) free energy lattice energy kinetic energy activation energy ionization energy 6 A sample of gallium metal is sealed inside a wellinsulated, rigid container The temperature inside the container is at the melting point of gallium metal What can be said about the energy and the entropy of the system Assume the insulation prevents any energy change with the surroundings (A) The total energy increases The total entropy will increase (B) The total energy is constant The total entropy is constant (C) The total energy is constant The total entropy will decrease (D) The total energy is constant The total entropy will increase (E) The total energy decreases The total entropy will decrease 7 When ammonium chloride dissolves in water, the temperature drops Which of the following conclusions may be related to this (A) The hydration energies of the ions are very high (B) Ammonium chloride produces an ideal solution in water (C) The heat of solution for ammonium chloride is exothermic (D) Ammonium chloride has a low lattice energy (E) Ammonium chloride is more soluble in hot water 8 Choose the reaction expected to have the greatest increase in entropy (A) (B) (C) (D) (E) H2O(g) H2O(1) C(s) + O2(g) CO2(g) Ca(s) + H2(g) CaH2(s) N2(g) + 3H2(g) 2 NH3(g) 2 KClO3(s) 2 KCl(s) + 3 O2(g)
1 the minimum energy required to initiate a reaction 2 the minimum energy required for a nonspontaneous reaction 3 The average_____________is the same for any ideal gas at a given temperature 4 the energy released when the gaseous ions combine to form an ionic solid 5 Given the following information: C(s) + O2(g) CO2(g) H = 3935 kJ H2(g) + (l/2) O2(g) H2O(l) H = 2858 kJ
C2H2(g) + (5/2) O2(g) 2 CO2(g) + H2O(l) H = 12998 kJ find the enthalpy change for: 2C(s) + H2(g) C2H2(g) (A) (B) (C) (D) (E) 4540 kJ 2270 kJ 00 kJ 2270 kJ 4540 kJ
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