Dynamic equilibrium

Chemistry Level 2

The gas nitrogen dioxide (NOX2)\big(\ce{NO2}\big) reacts in an exothermic reaction to the gas dinitrogen tetraoxide (NX2OX4)\big(\ce{N2O4}\big): 2NOX2(g)NX2OX4(g)+heat.\ce{2 NO2 (g) <-> N2O4 (g) + heat}. Since both forward reaction and reverse reaction take place, a dynamic equilibrium forms after some time. The equilibrium is determined by the law of mass action K=[NX2OX4][NOX2]2, K = \frac{\big[\ce{N2O4}\big]}{ \big[\ce{NO2}\big]^2}, where KK is the equilibrium constant. (In the gas phase, square brackets indicate partial pressure.)

How can the reaction be shifted to the product side, so that the equilibrium constant KK is increased?

×

Problem Loading...

Note Loading...

Set Loading...