Question 4 The following is a list of stresses that could be applied to a GASEOUS system at equilibrium a) Increasing the volume of the reaction vessel b) Increasing the pressure applied to the system c) decreasing the reaction temperature d) using a catalyst Which of the above stresses would i) change the magnitude of K? ii) ONLY shift the equilibrium position to re-establish K?

Question 4 The following is a list of stresses that could be applied to a GASEOUS system at equilibrium a) Increasing the volume of the reaction vessel b) Increasing the pressure applied to the system c) decreasing the reaction temperature d) using a catalyst Which of the above stresses would i) change the magnitude of K? ii) ONLY shift the equilibrium position to re-establish K?

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 40E: Consider the following system at equilibrium at 350K:CH4(g)+CCl4(g)2CH2Cl2(g)rH=18.8kJ. The...

See similar textbooks

Similar questions

The figures below represent the following reaction at equilibrium at different temperatures. A2(g)+3B2(g)2AB3(g)where squares represent atom A and circles represent atom B. Is the reaction exothermic?
Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
What is the difference between homogeneous equilibrium and heterogeneous equilibrium?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
Consider the following system at equilibrium at 350K:CH4(g)+CCl4(g)2CH2Cl2(g)rH=18.8kJ. The production of CH2Cl2(g) is favored by which of the following: a increasing the temperature; b increasing the pressure by changing the volume; c increasing the volume; d adding CH2Cl2, e removing CCl4 ?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.