Consider the following equilibrium: 2NO (g) + Cl, (g) =2NOCI (g) AG" = - 41. kJ Now suppose a reaction vessel is filled with 7.88 atm of chlorine (Cl,) and 9.01 atm of nitrosyl chloride (NOCI) at 1114. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCI tend to rise or fall? fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that yes be changed to a tendency to fall by adding NO? Similarly, if you said the no pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? |If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. O atm Round your answer to 2 significant digits.

Consider the following equilibrium: 2NO (g) + Cl, (g) =2NOCI (g) AG" = - 41. kJ Now suppose a reaction vessel is filled with 7.88 atm of chlorine (Cl,) and 9.01 atm of nitrosyl chloride (NOCI) at 1114. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCI tend to rise or fall? fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that yes be changed to a tendency to fall by adding NO? Similarly, if you said the no pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? |If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. O atm Round your answer to 2 significant digits.

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 99CP

See similar textbooks

Similar questions

. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
In Section 17.3 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 for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Indicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the reactants and products are all . If the volume of the system were doubled, all of the partial pressures would be . Would the system still be at equilibrium? Why or Why not?