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This set of questions addresses what would happen if a system at equilibrium N2(g) + 3 H2(g) → 2 NH3 (g) Consider the reaction: [NH,J [N,][H, When the reaction is at equilibrium, the ratio of concentrations, is CONSTANT and this constant is called Kc. For this entire set of questions, take the value of Kç for this reaction to be 16. [NH [N,][H,J When the reaction is NOT at equilibrium, the ratio can take on just about any value. For example, if we start with all reactants and zero products, then the ratio would equal zero. When not at equilibrium, we call this ratio Qc. It is referred to as the "reaction quotient". So, in summary: Qc can be any value when the reaction is not [NH,1 [N,][H,} [NH 1 [N,][H,F When the reaction is at equilibrium K. 16. at equilibrium. The value of Qc just depends on the concentrations of the R's %3D When the reaction is NOT at equilibrium, Oc #Constant %3D and P's in the reaction (1) If the concentrations of the reactants and products are as follows: [N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00 M .. is this system at equilibrium? Prove your answer by figuring out the value of Qc and seeing if it equals 16. If it does, the reaction is at equilibrium. mixture. %3D (2) Suppose you increase the concentration of N2 from 1.00 M to 2.00 M, leaving [H2] =1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way will the reaction go? First: What would LeChatelier's Principle say? To prove your answer, calculate the new reaction quotient, Qc. Is Qcgreater than, less than, or equal to Kc? (Circle one). If Qc is not equal to Kc, what would have to happen to make it equal 16?

This set of questions addresses what would happen if a system at equilibrium N2(g) + 3 H2(g) → 2 NH3 (g) Consider the reaction: [NH,J [N,][H, When the reaction is at equilibrium, the ratio of concentrations, is CONSTANT and this constant is called Kc. For this entire set of questions, take the value of Kç for this reaction to be 16. [NH [N,][H,J When the reaction is NOT at equilibrium, the ratio can take on just about any value. For example, if we start with all reactants and zero products, then the ratio would equal zero. When not at equilibrium, we call this ratio Qc. It is referred to as the "reaction quotient". So, in summary: Qc can be any value when the reaction is not [NH,1 [N,][H,} [NH 1 [N,][H,F When the reaction is at equilibrium K. 16. at equilibrium. The value of Qc just depends on the concentrations of the R's %3D When the reaction is NOT at equilibrium, Oc #Constant %3D and P's in the reaction (1) If the concentrations of the reactants and products are as follows: [N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00 M .. is this system at equilibrium? Prove your answer by figuring out the value of Qc and seeing if it equals 16. If it does, the reaction is at equilibrium. mixture. %3D (2) Suppose you increase the concentration of N2 from 1.00 M to 2.00 M, leaving [H2] =1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way will the reaction go? First: What would LeChatelier's Principle say? To prove your answer, calculate the new reaction quotient, Qc. Is Qcgreater than, less than, or equal to Kc? (Circle one). If Qc is not equal to Kc, what would have to happen to make it equal 16?

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Equilibrium v 2021 KS. Esquema Referências Correio Rever Ver Ajuda -12 A A Aa A AaBbCeDdl laBbCcD AatbCcdfe AaBbC daBbCeDdE Ênfase T Legenda I Normal Forte Subtítu ab x, x' A- . A- Parágrafo Estilos Tipo de Letra This set of questions addresses what would happen if a system at equilibrium is disturbed in different ways. Consider the reaction: N2(g) + 3 H2(g) → 2 NH3 (g) [NH,J [N,][H,j° When the reaction is at equilibrium, the ratio of concentrations, is CONSTANT and this constant is called Kc. For this entire set of questions, take the value of Kc for this reaction to be 16. [NHP [N,][H, When the reaction is NOT at equilibrium, the ratio can take on just about any value. For example, if we start with all reactants and zero products, then the ratio would equal zero. When not at equilibrium, we call this ratio Qc. It is referred to as the "reaction quotient". So, in summary: Qc can be any value when the reaction is not [NH1? When the reaction is at equilibrium K, : = 16. at equilibrium. The value of Qc just depends on the [NH,1 [N,][H,F When the reaction is NOT at equilibrium, Qc = #Constant concentrations of the R's and P's in the reaction (1) If the concentrations of the reactants and products are as follows: [N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00 M . is this system at equilibrium? Prove your answer by figuring out the value of Qc and seeing if it equals 16. If it does, the reaction is at equilibrium. mixture. (2) Suppose you increase the concentration of N2 from 1.00 M to 2.00 M, leaving [H2] =1.00 M and [NH3] = 4.00o M. Is the system at equilibrium now? If not, which way will the reaction go? First: What would LeChatelier's Principle say? To prove your answer, calculate the new reaction quotient, Qc. Is Qcgreater than, less than, or equal to Kc? (Circle one). If Qc is not equal to Kc, what would have to happen to make it equal 16? los Unidos) O Concentração
Transcribed Image Text:Equilibrium v 2021 KS. Esquema Referências Correio Rever Ver Ajuda -12 A A Aa A AaBbCeDdl laBbCcD AatbCcdfe AaBbC daBbCeDdE Ênfase T Legenda I Normal Forte Subtítu ab x, x' A- . A- Parágrafo Estilos Tipo de Letra This set of questions addresses what would happen if a system at equilibrium is disturbed in different ways. Consider the reaction: N2(g) + 3 H2(g) → 2 NH3 (g) [NH,J [N,][H,j° When the reaction is at equilibrium, the ratio of concentrations, is CONSTANT and this constant is called Kc. For this entire set of questions, take the value of Kc for this reaction to be 16. [NHP [N,][H, When the reaction is NOT at equilibrium, the ratio can take on just about any value. For example, if we start with all reactants and zero products, then the ratio would equal zero. When not at equilibrium, we call this ratio Qc. It is referred to as the "reaction quotient". So, in summary: Qc can be any value when the reaction is not [NH1? When the reaction is at equilibrium K, : = 16. at equilibrium. The value of Qc just depends on the [NH,1 [N,][H,F When the reaction is NOT at equilibrium, Qc = #Constant concentrations of the R's and P's in the reaction (1) If the concentrations of the reactants and products are as follows: [N2] = 1.00 M, [H2] = 1.00 M, [NH3] = 4.00 M . is this system at equilibrium? Prove your answer by figuring out the value of Qc and seeing if it equals 16. If it does, the reaction is at equilibrium. mixture. (2) Suppose you increase the concentration of N2 from 1.00 M to 2.00 M, leaving [H2] =1.00 M and [NH3] = 4.00o M. Is the system at equilibrium now? If not, which way will the reaction go? First: What would LeChatelier's Principle say? To prove your answer, calculate the new reaction quotient, Qc. Is Qcgreater than, less than, or equal to Kc? (Circle one). If Qc is not equal to Kc, what would have to happen to make it equal 16? los Unidos) O Concentração
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