A sample of N2O4(g) is placed in an empty cylinder at a certain temperature. After equilibrium is reached the total pressure is 2.3 atm and 13% (by moles) of the original N2O4(g) has dissociated to NO2(g). N2O4(g) NO2(g) a. Calculate the value of Kp for this dissociation reaction at this temperature. b. If the volume of the cylinder is increased until the total pressure is 1.0 atm (the temperature of the system remains constant), calculate the equilibrium pressure of N2O4(g) and NO2(g). c. What percentage (by moles) of the original N2O4 is dissociated at the new equilibrium position (total pressure = 1.00 am)?
A sample of N2O4(g) is placed in an empty cylinder at a certain temperature. After equilibrium is reached the total pressure is 2.3 atm and 13% (by moles) of the original N2O4(g) has dissociated to NO2(g). N2O4(g) NO2(g) a. Calculate the value of Kp for this dissociation reaction at this temperature. b. If the volume of the cylinder is increased until the total pressure is 1.0 atm (the temperature of the system remains constant), calculate the equilibrium pressure of N2O4(g) and NO2(g). c. What percentage (by moles) of the original N2O4 is dissociated at the new equilibrium position (total pressure = 1.00 am)?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 54QAP: Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When...
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A sample of N2O4(g) is placed in an empty cylinder at a certain temperature. After equilibrium is reached the total pressure is 2.3 atm and 13% (by moles) of the original N2O4(g) has dissociated to NO2(g).
N2O4(g) NO2(g)
a. Calculate the value of Kp for this dissociation reaction at this temperature.
b. If the volume of the cylinder is increased until the total pressure is 1.0 atm (the temperature of the system remains constant), calculate the equilibrium pressure of N2O4(g) and NO2(g).
c. What percentage (by moles) of the original N2O4 is dissociated at the new equilibrium position (total pressure = 1.00 am)?
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