Final answer:
To calculate the pressure of the gas mixture after the complete decomposition of N2O3, we'll use the equilibrium constant and initial partial pressures. By setting up an ICE table and solving the equilibrium constant expression, we can determine the partial pressures of the gases at equilibrium. The total pressure of the gas mixture after decomposition is the sum of the partial pressures.
Step-by-step explanation:
Given the initial partial pressures of N2O and O2, along with the equilibrium constant, we can set up an ICE table to determine the change in pressure for each gas.
Finally, we can calculate the equilibrium partial pressures of all three gases using the equilibrium constant and the initial partial pressures.
Using the equation N2O(g) + O2(g) ⇌ 2NO(g), the equilibrium constant expression can be written as
K = [NO]^2 / [N2O][O2].
Given the initial partial pressures of N2O (0.62 atm) and O2 (0.24 atm), as well as the initial pressure of NO (0.08 atm), we can substitute these values into the expression and solve for the equilibrium partial pressures.
After solving the expression, we find that the partial pressure of N2O at equilibrium is 0.62 atm, the partial pressure of O2 at equilibrium is 0.24 atm, and the partial pressure of NO at equilibrium is 2.52 atm.
Therefore, the pressure of the gas mixture after the complete decomposition of N2O3 is the sum of the partial pressures, which is 0.62 atm + 0.24 atm + 2.52 atm = 3.38 atm.