Chapter 13, Problem 108CP

Consider the decomposition equilibrium for dinitrogen pentoxide:

$2{\text{N}}_2{\text{O}}_5\left(g\right)\rightleftharpoons 4{\text{NO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

At a certain temperature and a total pressure of 1.00 atm, the N₂O₅ is 0.50% decomposed (by moles) at equilibrium.

a. If the volume is increased by a factor of 10.0. will the mole percent of N₂O₅ decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer.

b. Calculate the mole percent of N₂O₅ that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.