How would the equilibrium change if the temperature were increased in SO2(g) + NO2(g) NO(g) + SO3(g) + heat?A.The amount of NO and SO3 would increase.B.The equilibrium constant would decrease.C.Only the reaction rate would change.D.The amount of NO2 and SO2 would increase.

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.

Which way will the equilibrium shift, for the exothermic reaction below, if additional SO3(g) is added (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

Consider the equilibrium reaction represented by the equation: 2SO2(g) + O2(g) ⇌ 2SO3(g) ∆H = - 197 kJmol-1. At equilibrium, increase in the total pressure of the system brings aboutA. decrease in rate of the reaction of the systemB. decrease in temperature of the systemC. increase in temperature of SO3D. increase in concentration of SO2

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

What would happen if O2 were added to N2(g) + O2(g) 2NO(g) at equilibrium?A.More O2 would form.B.More N2 and NO would form.C.More NO would form.D.More N2 and O2 would form.