Question No. 6 Bookmark QuestionFor the reaction,A(g) + B(g) → C(g) + D(g), ΔH0 and ΔS0 are, respectively, –29.8 kJ mol–1 and –0.100 kJ K–1 mol–1 at 298K. The equilibrium constant for the reaction at 298K is

For the reaction    A(g)  +  B(g)  ⇋   2 C(g) the following equilibrium concentrations were found:[A(g)]  =  0.358 mol / L[B(g)]  =  0.216 mol / L[C(g)]  =  0.750 mol / LCalculate the value of the equilibrium constant Kc. Give 3 significant figures in your answer.

0.924 mole of A (g) is placed in a 1.00 liter container at 700 ° C, where it is 38.8 % dissociatedwhen equilibrium was established.3 A (g) 5 B (g) + 2 C (g)What is the value of the equilibrium constant, Kc, at the same temperature?

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

For the hypothetical reaction, A2(g) + B2(g) ⇌ 2AB(g), ΔrG and ΔrS are 20 kJ/mole and –20 JK–1 mol–1 respectively at 200 K. If given for the reaction ΔrCp is 20 JK–1 mol–1 then ΔrH of the reaction at 400 K is :-

What is the correct equilibrium constant expression or equation for the reactionH2(g) + Cl2(g) ⇋ 2HCl(g) Question 2Select one:a.b.c. d.