does the system reach equilibrium?what is the value of the equilibrium constant Kc? The particulate image above can be written in the following symbolic form asABIn which direction is equilibrium attained?Choose one:O A. In the forward directionO B. In the reverse direction○ C. The system does not reach equilibrium. The progress with time of a reaction system is depicted in the figure here. Red spheres represent the molar concentration of substance A, and bluespheres represent the molar concentration of substance B.Time

In the particulate image sequence, as time progresses, the number of red spheres (representing…

Answered: The particulate image above can be…

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter9: Chemical Reactions

Section: Chapter Questions

Problem 9.89EP

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Similar questions

. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
Complete the table below for the reaction 3A(g)+B(g)2C(g)
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations. Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the foll owing equation: A+BC+D a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. b. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. (a) Describe what happens in the first few minutes after the partition is opened. (b) What would you expect to see several hours later? (c) How is this system analogous to dynamic chemical equilibrium?
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations.
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
For the equilibrium reaction in Question 4, write the expression for the equilibrium constant. (a) How would this equilibrium constant change if the total pressure on the system were doubled? (b) How would the equilibrium constant change if the temperature were increased?
Classify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.
Indicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Addition of a product to the equilibrium mixture b. Increase in the systems total pressure c. Increase in the systems temperature d. Addition of both a reactant and a product to the equilibrium mixture
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Indicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Removal of a reactant from the equilibrium mixture b. Decrease in the systems total pressure c. Decrease in the systems temperature d. Addition of a catalyst to the equilibrium mixture
Equal amounts of two gases, A and B3, are placed in an evacuated container and react to form AB and B2. A(g)+B3(g)AB(g)+B2(g) The molecular scale diagram represents the relative amounts of each substance present once equilibrium is reached. Which of the following graphs best describes the progress of the reaction as it proceeds to equilibrium? Explain why the graph you chose must be the correct one.

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