H2 (g) + I2 (g) ---- 2HI (g) Kc = 2.35E-04 1.0 mol of H2 and 2.0 mol of I2 are placed in an empty 1.0 L flask What are the equilibrium concentrations of H2, I2, and HI? We must use stoichiometry to solve.

The equilibrium constant, K., for the following reaction is 5.10×10-6 at 548 K. NH,C(s)NH3(g) + HC(g) Calculate the equilibrium concentration of HCl when 0.501 moles of NH,CI(s) are introduced into a 1.00 L vessel at 548 K. [HCI] = |M

Question 41 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 x 10 at a certain temperature. If a solid sample of CaCrO4 dissolves in solution, what will the equilibrium concentration of Ca in the solution be? CaCrO.(s)= Ca (aq) + CrO (aq) NEXT Based on the given values, set up ICE table in order to determine the unknown. CaCrO-(s) Ca-(aq) CrO. (aq) Initial (M) Change (M) +2x +2x Equilibrium (M) 7.1 x 10-2x +2x +2x RESET 7.1 x 10 +2x -2x 7.1 x 10 +* 7.1 x 10-r 7.1x 10+ 2x 7.1x 10-2x

The equilibrium constant, Kc, for the following reaction is 1.80 × 10-4 at 298 K. NH4HS(s) NH3(g) + H₂S(g) If an equilibrium mixture of the three compounds in a 4.30 L container at 298 K contains 3.12 mol of NH4HS(s) and 0.310 mol of NH3, the number of moles of H₂S present is | mol.