For the reaction 4 PH, (g) = 6 H, (g) + P,(g) the equilibrium concentrations were found to be [PH,] = 0.250 M, [H, ] = 0.510 M, and [P] = 0.750 M. What is the equilibrium constant for this reaction? Ke =

The chemical equilibrium, 2A(g) = B(g) + C(g) has a Kc of 0.0460. Calculate the equilibrium concentrations of all three species if the starting concentrations are as follow:                                              [A] = 0.450 M, [B] = 0.330 M, and [C] = 0.330 M

Suppose a 250.mL flask is filled with 1.8mol of I2 and 1.4mol of HI. The following reaction becomes possible: +H2(g)+I2(g)--->2HI(g) The equilibrium constant K for this reaction is 1.03 at the temperature of the flask. Calculate the equilibrium molarity of I2 . Round your answer to two decimal places.

At a certain temperature, the reaction 2HF(g) e H2(g) + F2(g) has K. = 1.2 × 10-13. Does this reaction proceed far towards completion when equilibrium is reached? If 0.029 mol HF was placed in a 1.00 L container, and permitted to come to equilibrium, what would be the concentration of H2 and F2 in the container? Concentration of F2 at equilibrium = i M Concentration of H2 at equilibrium = i M