Section 7 - Chemical Equilibria all goo d. 7.6 0.500 mole of H2(g) and 0.500 moles of 12(g) are placed in a reaction vessel of volume 1.00 dm³ at 400 °C. H2(g) + I2(g) 2HI(g) Calculate the concentrations of H2, I2 and HI at equilibrium if the value of Kc at this temperature is 52.2.

11

Consider the following reaction: 2HI(g) = H2 (g) + I2 (g)   If 2.99 moles of HI(g) , 0.359 moles of H2, and 0.628 moles of I2 are at equilibrium in a 19.6 L container at 859 K, the value of the equilibrium constant, Kc , is .

A closed 1.00 L system initially containing 0.00200 mol H₂ and 0.00500 mol 1₂ at a given temperature is allowed to reach equilibrium Analysis of the equilibrium mixture shows that the amount of HI present at equilibrium is 0.00371 mol. Calculate the Kc at this temperature for the reaction. State whether the equilibrium is product-favored or reactant- favored at this temperature. H₂(g) +1₂(g) 2H1(g) Kc 31: The equilibrium is product-favored. Kc 31: The equilibrium is reactant-favored. Kc 0.032; The equilibrium is reactant-favored. Kc - 0.032; The equilibrium is product-favored.

A2

The equilibrium constant, K,, for the following reaction is 2.74 at 1.15x1o3K. 2503(g) 2s02(g) + 02(g) If an equilibrium mixture of the three gases in a 16.5 L container at 1.15×103K contains soz at a pressure of 1.62 atm and So, at a pressure of 1.04 atm, the equilibrium partial pressure of O, is atm.

12.) A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) = N2(g) + 3H2(g) At equilibrium, the mixture contained to following concentrations: [H2] = 0.0283 M, [N2] = 0.00944 M,[NH3] = 0.101 M. What is Kp at this temperature?

Hh.53.

At a certain temperature, 0.760 mol SO, is placed in a 2.50 L container. 2 SO,(g) = 2 SO2(g) + O,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke

The equilibrium constant Kc for the reaction,I2(g) + Br2(g) <-----> 2 IBr(g) is 26 at 425 K. What is the value of Kc for the equilibrium,1/2 I2(g) + 1/2 Br2(g) <-----> IBr(g) at 425 K?