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.

For the reaction:2 A (g) B (g) + C (g)at 900 ° C, Kc is 1.40 x 10 -3. If 0.780 mole of A (g) and 0.244 mole each of B (g) and C (g) are mixed in a1.00 liter container at 900 ° C, what are the concentrations of A, B, and C at equilibrium?

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?

Samples of A (1.0 mol) and B (3.5 mol) are placed in a 1 L container and the following reaction takes place:A(g)  +  B(g)  ⇄ 2C(g)  At equilibrium, the concentration of A is 0.6 M.  What is the value of K to 2 d.p?

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

A solution is made by mixing 30.0 mL of 0.150M (mol/L) compound A with 25.0 mL of 0.200M (mol/L) compound B. At equilibrium, the concentration of C is 0.0454M. Calculate the equilibrium constant, K, for this reaction.A (aq) + 2B (aq) <---> C (aq)The initial concentrations of A and B are not 0.150 M and 0.200 M