Textbook Question
Consider the reaction 2 NO2(g) → N2O4(g). (a) Using data from Appendix C, calculate ΔG° at 298 K. (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.40 atm and 1.60 atm, respectively.
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Ch.19 - Chemical Thermodynamics
Chapter 19, Problem 79
Use data from Appendix C to calculate the equilibrium constant, K, and ΔG° at 298 K for each of the following reactions: (a) H2(g) + I2(g) ⇌ 2 HI(g) (b) C2H5OH(g) ⇌ C2H4(g) + H2O(g) (c) 3 C2H2(g) ⇌ C6H6(g)
Verified step by step guidance1
Step 1: Identify the standard Gibbs free energy of formation (ΔG°f) for each reactant and product from Appendix C for each reaction at 298 K.
Step 2: Calculate the standard Gibbs free energy change (ΔG°) for each reaction using the formula: ΔG° = Σ(ΔG°f of products) - Σ(ΔG°f of reactants).
Step 3: Use the relationship between ΔG° and the equilibrium constant (K) given by the equation: ΔG° = -RT ln(K), where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin (298 K).
Step 4: Rearrange the equation from Step 3 to solve for the equilibrium constant (K): K = e^(-ΔG°/RT).
Step 5: Substitute the calculated ΔG° from Step 2 into the equation from Step 4 to find the equilibrium constant (K) for each reaction.
Related Practice
Textbook Question
Consider the reaction 3 CH4(g) → C3H8(g) + 2 H2(g). (a) Using data from Appendix C, calculate ΔG° at 298 K.
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Textbook Question
Consider the reaction 3 CH4(g) → C3H8(g) + 2 H2(g). (b) Calculate ΔG at 298 K if the reaction mixture consists of 40.0 atm of CH4, 0.0100 atm of C3H8(g), and 0.0180 atm of H2.
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Textbook Question
Using data from Appendix C, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K: (a) NaHCO3(s) ⇌ NaOH(s) + CO2(g)
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Textbook Question
Consider the decomposition of barium carbonate: BaCO3(s) ⇌ BaO(s) + CO2(g) Using data from Appendix C, calculate the equilibrium pressure of CO2 at (a) 298 K.
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Textbook Question
Consider the decomposition of barium carbonate: BaCO3(s) ⇌ BaO(s) + CO2(g) Using data from Appendix C, calculate the equilibrium pressure of CO2 at (b) 1100 K.
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