Consider the following reaction (assume an ideal gas mixture): 2NOBr(g) 2NO(g)+ Br 2 (g)A 1.0-liter vessel was initially filled with pure NOBr,at a pressure of 4.0 atm,at 300 K.
-After equilibrium was reached,the volume was increased to 2.0 liters,while the temperature was kept at 300 K.The result of this change was

Question

Consider the following reaction (assume an ideal gas mixture): 2NOBr(g)  2NO(g)+ Br 2 (g)A 1.0-liter vessel was initially filled with pure NOBr,at a pressure of 4.0 atm,at 300 K.
-After equilibrium was reached,the volume was increased to 2.0 liters,while the temperature was kept at 300 K.The result of this change was

Quizplus · Accepted Answer

Increasing the volume of a system at equilibrium (while keeping temperature constant) decreases the pressure, causing the equilibrium to shift in the direction that produces more moles of gas. This is described by Le Chatelier's principle. Without specific reaction details, the general response to an increase in volume is a shift to the side with more gas molecules, which is often interpreted as a shift to the right.

Consider the Following Reaction (Assume an Ideal Gas Mixture): 2NOBr(g)