A sample of N2O4(g) is placed in an empty cylinder at 25oC. After equilibrium is reached, the total pressure is 1.5 atm, and 16% (by moles) of the original N2O4(g) has dissociated to NO2(g).
a. Calculate the value of Kp for this dissociation reaction at 258C.
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(g) is dissociated at the new equilibrium position (total pressure = 1.00 atm)?

  • CreatedMay 05, 2015
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