If one starts with pure NO₂(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO₂(g) $\rightleftharpoons$ 2NO(g) + O₂(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO₂.

Question

Quizplus · Accepted Answer

The equilibrium partial pressure of NO₂ is 0.152 atm because the total pressure increases from 0.500 atm to 0.674 atm, indicating that the reaction proceeds in the forward direction to form more NO and O₂. Therefore, the partial pressure of NO₂ must decrease.

If One Starts with Pure NO2(g) at a Pressure of 0.500

If One Starts with Pure NO₂(g) at a Pressure of 0.500