At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)+2B(g)−⇀↽−4C(g)Kc=1.53×1019 If, at this temperature, 1.00 mol of A and 3.50 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium?

The equilibrium constant for the reaction shown below is 61.2 H, (g) + Br, (g) = 2HB1(g) Write an expression for the equilibrium constant, K What is the equilibrium concentration of Br2, if [HBr]=0.48 M and [H2] = 0.26 M at equilibrium?

At a certain temperature, 0.3011 mol of N₂ and 1.781 mol of H₂ are placed in a 4.00 L container according to the following equation: N₂(g) + 3H2(g) + 2NH3(g) At equilibrium, 0.1401mol of N₂ is present. Calculate the equilibrium constant.

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kç. 3 A(g) + 2 B(g) = 4 C(g) K = 1.33 x 102' If, at this temperature, 1.70 mol of A and 4.00 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = M [B] = M [C] = M

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 5.40x10-4 moles of NH3(g), 0.450 moles of N₂, and 0.215 moles of H₂ are at equilibrium in a 15.1 L container at 846 K, the value of the equilibrium constant, K, is