Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system?2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g)The equilibrium constant will increase.The reaction will shift to the left in the direction of reactants.No effect will be observed.The equilibrium constant will decrease.The reaction will shift to the right in the direction of products.

16.      In which of the following equilibrium systems would an increase in volume (at constant temperature) cause the reaction to shift to the right?   *A. N2O4(g) 2NO2(g)B. N2(g) + 3H2(g) 2NH3(g)C. H2(g) + Cl2(g) 2HCl(g)D. Answers a and b are correct.

For the following equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen to the concentrations of each gas if the pressure is increased?SO2 and O2 will decrease; SO3 will increaseSO2, O2 and SO3 will all decreaseSO2, O2 and SO3 will all increaseSO2 and O2 will increase; SO3 will decrease

Which way will the equilibrium shift, for the exothermic reaction below, if the pressure is increased by decreasing the volume (and everything else is held constant)?2SO2(g) + O2(g)  2SO3(g)Group of answer choicesTo the left (more reactants)To the right (more products)It will not shift

How would the equilibrium of the reaction below be affected if the temperature increased?A.The concentrations of O2, SO2, and SO3 would increase.B.The concentrations of O2, SO2, and SO3 would decrease.C.The concentration of SO3 would increase.D.The concentrations of O2 and SO2 would increase.

Use Le Chatelier’s Principle to predict how the addition of more SO3 gas will shift the equilibrium of this reaction:2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)Question 2Select one:a.shift right (in the forward direction) and then left (in the reverse direction)b.shift right (in the forward direction) to make more productsc.shift in equilibrium not caused by adding more SO3d.shift left (in the reverse direction) to make more reactants