Which of the following equilibria is shifted to the right as a result of an increase in pressure?
H2(g) + I2(g) 2HI(g)
2NO2(g) N2O4(g)
PCl5(s) PCl3(s) + Cl2(g)
2O3(g) 3O2(g)
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it's b cos increase in pressure favours side dt proceed wit a decrease in volume.... We have 2 volumes in d reactant n 1 volume at d product side thus increase in pressure will favour side wit lower volume. D equilibrium will shift to d right.
The equilibrium that is shifted to the right as a result of an increase in pressure is the one that has fewer gas molecules on the right side of the equation. This is because an increase in pressure will favor the side of the equation with fewer gas molecules, which will decrease the total number of moles of gas in the system and thus decrease the pressure.
Therefore, the correct answer is:
B. 2NO2(g) N2O4(g)
This is because there are fewer gas molecules on the right side of the equation (1) than on the left side (2). When pressure is increased, the equilibrium will shift to the right to decrease the total number of moles of gas in the system, favoring the formation of N2O4(g)
