Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
Answer 1 and 2 Asap please
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
Expert Solution
steps

Step by step

Solved in 4 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Quality Assurance and Calibration Methods
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS