CHEM 1212 1st Edition Lecture 14 Outline of Last Lecture - Practice Problems- Quadratic Equation- Avoiding the Quadratic EquationOutline of Current Lecture - In-class examplesCurrent Lecture- Ex: Suppose 0.086 moles of Bromine, Br2, is placed in a 1.26-L flask and heated to 1756K,a temperature at which the halogen dissociates to atoms.o Br2(g)  2Br(g)o If Br2 is 3.7% dissociated at this temperature, calculate Kco Answer: 3.8x10-4o <1 = reactant favored reaction- Ex: Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants.o SO2(g) + 1/2O2(g)  SO3(g) K1o 2SO3(g)  2 SO2(g) + O2(g) K2o Which of the following expressions relates K1 to K2?A. K2 = K12B. K22 = K1C. K2 = K1D. K2 = 1/K1E. K2 = 1/K12- Ex: A 15-L flask at 300K contains 64.4 g of a mixture of NO2 and N2O4 in equilibrium. What is the total pressure in the flask?o 2NO2(g)  N2O4(g) Kp = 7.1o Left this problem for us to solve; might see it later (EOC problem)- Ex: At 2300K the equilibrium constant for the formation of NO(g) is 1.7x10-3o N2(g) + O2(g)  2NO(g)These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.o If the initial concentration of nitrogen gas and oxygen gas are 0.88 mol/L and theinitial concentration of nitrogen monoxide is 0.062 mol/L, what are the equilibrium concentrations of all species?o Answer: [N2] = [O2] = [NO] = Left this for us to solve for practice as well (in-chapter example)- Le Chatelier’s Principleo Given the reaction N2(g) + 3H2(g)  2NH3(g) ΔH = -222.6 kJ/mol-rxn; Kc = 0.16 @ 450°C What happens when more nitrogen gas is introduced to a system already at equilibrium?A. Reactants are consumed and products are produced to reach a new equilibrium conditionB. Products are consumed and reactants are produced to reach a new equilibrium conditionC. Nothing changes What happens when some nitrogen gas is removed from a system alreadyat equilibrium?Same choices as above; Answer: B What happens when more ammonia gas is introduced to a system alreadyat equilibrium?Same choices as above; Answer: B What happens when the temperature is increased for a system already at equilibrium?Answer: B What happens when the volume is reduced for a system already at equilibrium?Answer: A- Consider the isomerization of butane with an equilibrium constant of K=2.5o Butane  isobuteneo The system is originally at equilibrium with [butane] = 1.0M and [isobutene] = 2.5 Mo If 0.50 mol/L of isobutene is suddenly added and the system shifts to a new equilibrium position, what is the equilibrium concentration of