Ccan you help me every step by step? Can you help me with number 2 part A and number 2 part B? Le Chatelier's Principle and Equilibrium Shifts1. If the reaction below is initially at equilibrium, and then each of the following changes aremade, predict which direction the reaction rate will be fastest until equilibrium is once againestablished: forward, reverse, or no change.Reactant2COg+O2g) # 2 CO2(g)a. The concentration of O₂ is increased. -forward, reactantb. The concentration of CO₂ is decreased? forwardl, eactantc. The concentration of oxygen gas is decreased. reverse, productProduct2. If the reaction below is initially at equilibrium, and then each of the following changes aremade, predict which direction the reaction rate will be fastest until equilibrium is once againestablished: forward, reverse, or no change.ReactantC(s) + H₂O(g)a. adding H₂0) forward.b. removing H₂ forwarddecrea. adding PC13 reverseincreasc b. removing Ch₂ forwardincreast c. removing PC13 forwarddecreased. adding Cl₂ reverseProductCO(g) + H2(g)3. If the reaction below is initially at equilibrium, and then each of the following changes aremade, predict which direction the reaction rate will be fastest until equilibrium is once againestablished: forward, reverse, or no change.ReactantProductPC15)PC13(g) + Cl2(g) Change Made to a Reactionthat was at Equilibrium:Increase the concentration of a reactant.Increase the concentration of a product.Decrease the concentration of a reactant.Decrease the concentration of a product.Response:Rate of the forward reaction becomes greater than the rateof the reverse reaction until equilibrium is reestablished.Rate of the reverse reaction becomes greater than the rateof the forward reaction until equilibrium is reestablished.Rate of the forward reaction becomes less than the rate ofthe reverse reaction until equilibrium is reestablished.Rate of the reverse reaction becomes less than the rate ofthe forward reaction until equilibrium is reestablished.

Solving question 2a and 2b as asked. Predict the rate of reaction ( forward, backward or no effect)…

2. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. Reactant C(s) + H₂O(g) a. adding H₂O(g) forward. b. removing H₂ forward Product CO(g) + H2(g)

2. If the reaction below is initially at equilibrium, and then each of the following changes are made, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. Reactant C(s) + H₂O(g) a. adding H₂O(g) forward. b. removing H₂ forward Product CO(g) + H2(g)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 9RQ: What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at...

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. 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?
Consider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of N2O4 and NO2 as equilibrium is approached. Describe how the rates of the forward and reverse reactions change as the mixture approaches dynamic equilibrium. Why is this called a dynamic equilibrium?
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. 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. h. 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.
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchanged
. For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?
Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volume
Phosphorus pentachloride decomposes at elevated temperatures. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.120 g of PCl5, 3.845 g of PCl3, and 1.787 g of Cl2 in a 10.0-L flask. If you add 1.418 g of Cl2, how will the equilibrium be affected? What will the concentrations of PCl5, PCl3, and Cl2 be when equilibrium is reestablished?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.