Chem1011GeneralChemistryII_EquilibriumandLeChteliersPrinciple_134692

Copyright 2024 - Science Interactive | https://scienceinteractive.com The state of chemical equilibrium occurs when the concentrations of _____. all reactants and all products remain constant products is less than the concentration of reactants reactants is greater than the concentrations of products Chemical equilibrium occurs when free energy exists in the _____. highest possible value lowest possible value Generally, if the value of K is greater than 1, we say that the reaction favors the _____ and if the value of K is less than 1, the reaction favors the _____. products; reactants reactants; products Neither reactants nor products are favored. The equilibrium position of a reaction requires the variables of _____, _____, and _____ to remain constant. color, pressure, concentration concentration, time, temperature pressure, temperature, concentration time, color, temperature Le Châtelier’s principle includes the idea that a change imposed on a chemical system will cause the system to find a new chemical equilibrium where free energy exists at the highest possible value. True False

Copyright 2024 - Science Interactive | https://scienceinteractive.com Qc = [NH ] / [N ] [H ] Qc = (1.0 x 10 M) / (4.0 M) (2.5 x 10 M) Qc = 1.6 x 10 Qc < Kc Chemical system will shift right and produce more NH . Consider the chemical reaction: N + 3H yields 2NH . If the concentration of the reactant H was increased from 1.0 x 10 M to 2.5 x 10 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10 , with initial concentrations as follows: [H ] = 1.0 x 10 M, [N ] = 4.0 M, and [NH ] = 1.0 x 10 M. 2 2 3 2 -2 -1 -2 2 -2 2 3 -4 3 2 2 2 3 -4 2 -1 3 -7 3 Qc = [NH ] / [N ] [H ] Qc = (1.0 x 10 M) / (4.0 M) (2.7 x 10 M) Qc = 127 Qc > Kc Chemical system will shift left and produce more N and H . If the concentration of the reactant H was decreased from 1.0 x 10 M to 2.7 x 10 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. 2 -2 -4 3 2 2 2 3 -4 2 -4 3 2 2

Copyright 2024 - Science Interactive | https://scienceinteractive.com Data Table 3: Ferric Ferrocyanide Competency Review Color of Potassium Ferrocyanide Color of Ferric Ferrocyanide Color of Potassium Ferrocyanide Number of Drops of NaOH to Shift Equilibrium Position Color of Potassium Ferrocyanide Observations when Equilibrium is Shifted Pale yellow Dark blue Pale yellow 1 Pale yellow Color becomes transparent, pale yellow color, less viscous/more watery, brown particles in solution A chemical system is in equilibrium when free energy exists at _____. the highest possible value the lowest possible value equal proportions During a chemical reaction, if the concentration of reactants and products doesn't change, the reaction has likely stopped. True False

Copyright 2024 - Science Interactive | https://scienceinteractive.com This is an exothermic reaction since its enthalpy is a negative value. That means that increasing temperature is akin to increasing the amount of products in the reaction. Increasing products will shift the equilibrium to the left to produce more C2H2. There are 3 moles of reactants to 1 mole of product. Decreasing the pressure will cause the equlibrium to shift toward the reactants and produce more C2H2. Increasing volume also accomplishes this since higher volume means lower pressure. Removing C2H2 or H2 as it is being produced will reduce the concentration of reactants which will prompt the equilibrium to shift left ot produce more C2H2. Assume that you are in charge of a designing a process to produce acetylene (C H ) from ethane (C H ), which is the reverse of the reaction shown above. Use your knowledge of equilibrium to suggest a set of conditions that would maximize the concentration of acetylene (C H ) at equilibrium. Assume that it is possible to add or remove any of the three components of this system and to change the general conditions of the reaction (pressure, temperature, volume). Use your knowledge of equilibrium to suggest a set of conditions that would maximize the concentration of acetylene (C H ) at equilibrium. 2 2 2 6 2 2 2 2