Consider the chemical system:2 NO(g) + Br2(g)  ⇋ 2 NOBr (g)K = 2.0  How do the equilibrium concentrations of the reactants compare to the equilibrium concentration of the product?Question 2Select one:a.You can't tell from the information givenb.They are much higherc.They have to be exactly equald.They are about the same order of magnitudee.They are much lower

Consider the chemical system: A(g) + 3 B(g)  ⇋  C (g)K = 6 x 1012   How do the equilibrium concentrations of the reactants compare to the equilibrium concentration of the product?Question 1Select one:a.Reactant and product concentrations have to be exactly equal at equilibriumb.You can't tell from the information given because of the stoichiometryc.Reactant concentrations are much lower, products dominate at equilibrium.d.Reactant and product concentrations are about the same order of magnitudee.Reactant concentrations are much higher, reactants dominate.

a. At a certain temperature, Kc is 4.13 x 10 -2 for the equilibrium:2 IBr (g) I2 (g) + Br2 (g)Assume that equilibrium is established at the above temperature by adding only IBr (g) to the reactionflask. What are the concentrations of I2 (g) and Br2 (g) in equilibrium with 0.0124 moles/liter of IBr(g) ?

TRUE OR FALSE: At equilibrium, the concentrations of reactants and products are equal.

2. Given the following information, use an ICE table to calculate the equilibrium concentration of BrCl.[Br2]i = 0.225[Cl2]i = 0.125Kc = 0.0875Br2(g)+ Cl2(g) ⇌ 2BrCl(g)0.104 M0.050 M0.204 M0.153 M

For the reaction system A2(g) + B2(g) ⇋ 2AB(g)the equilibrium constant Kc= 2.8A system using this reaction was being tried in a 1.00 L reactor. It was charged with 0.30 mol A2, 0.10 mol B2 and 0.50 mol AB.The system was allowed to come to equilibrium. Which statement below describes the system coming to equilibrium?(Note: in the answers, Q refers to the reaction quotient, K refers to the equilibrium constant).Question 6Select one:a.The reaction goes to the right, more products will form because Q < Kb.The reaction goes to the left, more reactants will form because Q < Kc.The reaction goes to the right, more products will form because Q > Kd.It is not possible to predict in which direction the system will travel to arrive at equilibrium.e.The reaction goes to the left, more reactants will form because Q > K