Consider the following reaction at equilibrium Co(g) + H,O(g) = co.(g) + H,(g) If CO(g) is removed, in which direction will the equilibrium shift? A) reactants B) products C) no change

Consider the reversible reaction N2 + 3H2 = 2NH3 If one adds extra H2 to an equilibrium mixture containing N2, H2 and NH3: a) more N2 will be formed b)  more NH3 will be formed  c)  no change will take place   d)  new compounds will be formed If one adds a catalyst to an equilibrium mixture containing N2, H2 and NH3: a) more H2 will be formed b)  more NH3 will be formed  c)  no change will take place   d)  new compounds will be formed The ∆H for this reaction is (-)5.7 kilojoules per mole. If one increases the temperature of an equilibrium mixture containing N2, H2 and NH3: a) more N2 will be formed b)  more NH3 will be formed  c)  no change will take place   d)  new compounds will be formed Increasing the pressure of an equilibrium mixture containing N2, H2 and NH3: a) more N2 will be formed b)  more NH3 will be formed  c)  no change will take place   d)  new compounds will be formed

Which K value below is consistent with an equilibrium system in which the reactants are favored?  A) K=1  B) K=1.8 x 103   C) K= 3.7 x 10-8  D) K= 500

7:42 Question 45 of 50 Submit The reaction of NO(g) + Cl₂(g) = NOCI(g) + Cl(g) is found to have an equilibrium constant of 1.1x10³ at a particular temperature. What does this mean? A) At equilibrium, there is a much higher concentration of reactants than products. B) At equilibrium, there is a much higher concentration of products than reactants. C) At equilibrium, there is an equal concentration of reactants and products. D) At equilibrium, the relative concentrations of reactants and products depends on the initial concentrations. Tap here or pull up for additional resources