Acttivity 4 Numbers 1 and 2 2. 2ZnS + 302 ( = 2ZnO + 2SO2Processing Question1. What factors can affect systems in equilibrium?INTEGRATIONReflection Guide1. How do you value academic proficiency in answering this module?INTERVENTIONPost - assessmentIt's now time to assess your learning. If you do well, you may move on to the next lesson.If your score is not at the expected level, you may talk to your subject teacher to go back withthe lesson and for you to be given remedies to cope up and understand the lesson.Directions: Read the following questions below. Circle the letter that corresponds to the correct answer.1. In case of nonspontaneous reaction, the reaction favoured isC. both forward and reverseD. reaction stopsA. ForwardB. Reverse2. In which of the following physical states does a given substance have the highest entropy?A. SolidB. GasC. liquidD. entropy is the same3. What are the two factors that determine whether a reaction is spontaneous or nonspontaneous?A. Entropy and disorderB. Entropy and enthalpy changeC. electron configuration and chargeD. energy and the heat of reaction4. The amount of disorder in a system is measured by itsA. Activation energyB. EntropyC. equilibrium positionD. Keq5. Which of the following refers to all spontaneous processes?A. Are exothermicB. Are endothermicC. involve an increase in entropyD. release free energyPage | 8 2.PNH3Kp PN2PH2%3D3.[N21 [H2]3Heterogeneous EquilibriaA heterogeneous equilibrium consists of reactants and products that exist in different phases. An example is theCACO3 (9) = Ca0 9 + CO2 (3)In a heterogeneous equilibrium, pure solid and liquid substances do not appear in the equilibrium constantexpression. The molar concentrations of these substances are always constant (having a value equal to 1). The values arethen not incorporated in the equilibrium constant expressions. For the calcium carbonate equilibrium reaction, the KK = [CO2]K, = Pco2%3D%3DpueLe Chatelier's PrincipleV A system will adjust to regain its equilibrium if stress is applied to it.Le Chatelier's principle states that when stress is introduced into a system in equilibrium, the system will adjustto relieve the stress and regain equilibrium. The stress is relieved as the reaction shifts either to the left (reverse) or to theright (f of the reversible reaction.One factor that can affect systems in equilibrium is the change in the amount of either the reactants or theproducts. Adding more reactants to a reaction that is already in equilibrium will cause it to shift to the right. Adding moreproducis will favour the reverse reaction.Activity 4 Ke and K,Directions: Write the equilibrium constant expression (K. and K, ) for the following reactions:1. 2SO2 (2)+ 02 ( =e 2SO3 (g)Page | 7

Equilibrium constant in terms of concentration ( Kc ) is the ratio of concentration of products to…

Answered: Activity 4 Kc and K, Directions: Write…

Activity 4 Kc and K, Directions: Write the equilibrium constant expression (Ke and K, ) for the following reactions: 1. 2SO2 (2 + 02 g = 2SO3 ()

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.ACP

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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) A )Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc = _____/_____ = _____ Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the concentration of O₂ at equilibrium. [O₂]eq = _____M
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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc= (_______) / (_______) = (______) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. N₂(g) + O₂(g) ⇌ 2 NO(g) Initial (M) Change (M) Equilibrium (M) Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the…
In the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species, kx, kp and ∆G0
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For this heterogeneous system 2A(aq)+3B(g)+C(l)↽−−⇀2D(s)+3E(g) the concentrations and pressures at equilibrium are [A]=1.35×10−2 M, ?B=8.62×103 Pa, [C]=14.93 M, [D]=12.55 M, and ?E=5.86×104 torr. Calculate the thermodynamic equilibrium constant, ?. please type in words don't image upload thank you.
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https://youtu.be/MzpmUHdwLr0 1) Write the expression for the equilibrium constant, Kc , for the following system: CaCO3(s) ⇄⇄ Ca2+(aq) + CO32–(aq) a. During ocean acidification the availability of carbonate ions has decreased and the above system is no longer in equilibrium. Will the resulting reaction quotient, Qc, be larger or smaller than the equilibrium constant, Kc? b. Consider your answers to the above questions. In terms of the calcium carbonate equilibrium system, and Qc and Kc, explain why the pteropod's shell dissolves in an acidified ocean.