G Answer all the questions in the spaces provided 1 (a) N₂(g) O₂(g) 2NO (g) AH298+180 kJ mol-¹ From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst

G Answer all the questions in the spaces provided 1 (a) N₂(g) O₂(g) 2NO (g) AH298+180 kJ mol-¹ From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N₂ (e) Adding a catalyst

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.54PAE: Consider the following system: 4NH 3 ( g )+ 3O 2 ( g ) N 2 ( g )+ 6H 2 O( l ) H=1530.4kJ (a) How...

See similar textbooks

Similar questions

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
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?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
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?
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 following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
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?
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-.
Red phosphorus is formed by heating white phosphorus. Calculate the temperature at which the two forms are at equilibrium, given white P: H f =0.00 kJ/mol; S =41.09 J/mol K red P: H f =17.6 kJ/mol; S =22.80 J/mol K
Consider the following system: 4NH 3 ( g )+ 3O 2 ( g ) N 2 ( g )+ 6H 2 O( l ) H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by (1) removing O2(g) (2) adding N2(g)? (3) adding water? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When equilibrium is established, a 2.5-L reaction vessel at 125C contains 15.0 g of R, 4.3 atm of X2, and 0.98 atm of X2R. (a) Calculate K for the reaction at 125C. (b) The mass of R is doubled. What are the partial pressures of X2 and X2R when equilibrium is reestablished? (c) The partial pressure of X2 is decreased to 2.0 atm. What are the partial pressures of X2 and X2R when equilibrium is reestablished?