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 for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.108PAE: 12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant...
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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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