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07:32Consider the equilibrium N2(π) + O2(π) + Br2(π) β 2 NOBr(π) Calculate the equilibrium constant πΎπ for this reaction, given the following information at 298 K:
2 NO(π) + Br2(π) β 2 NOBr(π) πΎπ = 2.02
NO(π) β N2(π) + O2(π) πΎπ = 2.1Γ1030
The equilibrium 2 NO(π) + Cl2(π) β 2 NOCl(π) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate πΎπ for this reaction at 500.0 K.
The equilibrium 2 NO(π) + Cl2(π) β 2 NOCl(π) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(π) + H2(π) β CO(π) + H2O (π) (d) Calculate πΎπ for the reaction.
(a) If Qc < Kc, in which direction will a reaction proceed in order to reach equilibrium?
(b) What condition must be satisfied so that Qc = Kc?
