Which of the following equilibria is shifted to the right as a result of an increase in pressure?

When pressure is increased, the equilibrium will shift to the side with fewer moles of gas molecules. - In the first option, the number of gas molecules remains the same on both sides of the equation, so there will be no shift in equilibrium. - In the second option, the number of gas molecules decreases from four to two as the reaction proceeds to the right, so an increase in pressure will shift the equilibrium to the right. - In the third option, the number of gas molecules increases from one to two as the reaction proceeds to the right, so an increase in pressure will shift the equilibrium to the left. - In the fourth option, the number of gas molecules decreases from five to three as the reaction proceeds to the right, so an increase in pressure will shift the equilibrium to the right. Therefore, the equilibrium that will shift to the right as a result of an increase in pressure is the one described in the second option: 2NO2(g) ⇌ N2O4(g).