The equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K. NH4I(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.05 L container at 673 K contains 2.71 mol of NH4I(s) and 0.262 mol of NH3, the number of moles of HI present is moles.

KINETICS AND EQUILIBRIUM Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant X for the following reaction is 0.0099: CO(g) + H₂O(g) = CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 0.60 mol of CO₂ and 0.60 mol of H₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. CO₂(g) + H₂(g) → CO(g) +H₂O(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 3 CO(g) +3H₂O(g) 3 CO₂(g)+ 3H₂(9) There will be very little CO and H₂O. There will be very little CO₂ and H₂. Neither of the above is true. K = 0 K = 0 □ x10 X 3/5

The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH3(g) + H₂S(g) NH4HS(s) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.366 mol NH4HS, 1.34×10- M NH3 and 1.34×10-² M H₂S. If the concentration of NH3(g) is suddenly increased to 2.41x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] = ΣΣ M

The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH,Cl2(g) ? CH,(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43x10-2 M CH,Cl,, 0.176 M CH, and 0.176 M CCL. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.124 mol of CH,(g) is added to the flask? [CH,Cl,] = M [CH4) M [CCL] M