Nitrogen and oxygen gases react reversibly to produce gaseous N2O4 in a 4.00 L container being held at 278 K. 2.00 mols of each reactant and 1.00 mol of the product are initially placed into the...

Extracted text: Nitrogen and oxygen gases react reversibly to produce gaseous N2O4 in a 4.00 L container being held at 278 K. 2.00 mols of each reactant and 1.00 mol of the product are initially placed into the container, and once the reaction establishes equilibrium, the molarity of oxygen gas is measured as 0.150 M. Answer the questions below.


Extracted text: Let's go back to the original equilibrium position established by the reaction, with the equilibrium molarity for oxygen gas as 0.150 M. With the temperature still held at 278 K, the total volume of the reaction is changed and the new equilibrium molarity for oxygen gas is found to be 0.215 M. Was the volume of the container changed to 2.00 L or 6.00 L? Circle and explain your choice below. 2.00 L 6.00 L