File: EquilCha. Equilibrium and Le Chatelier's Principle. (pp.126,128,125,134,136,286,288,290,292)Page 1261.An equilibrium mixture at 425oC is determined to consist of 1.83 x 10-3 mole/ liter of H2, 3.13 x 10-3 mole/ liter of I2, and also 17.7 x 10mole/ liter of HI. Calculate the equilibrium constant. -3 2. An equilibrium mixture at 424oC consists of 4.79 x 10-4mole/ L of H2, 4.79 x 10-4 mole/ L of I2, and 3.53 x 10-3mole/ L of HI. Determine the equilibrium constant.3.When 0.40 mole of PCl5 is heated in a 10 liter container an equilibrium is established in which 0.25 moles of Cl2 is present.PCl5 PCl3 + Cl(a) What is the number of moles of PCl5 and PCl3 at equilibrium? (b) What are the equilibrium concentrations of all three components? (c) What is the Keq?Hint: The equation shows that for each mole of Cl2 formed, 1 mole of PClis formed and 1 mole of PCl5 is consumed.23 5. When 1.00 mole of NH3 and 0.40 mole of N2 gas are placed in a 5 liter container and allowed to reach equilibrium at a certain temperature, it is found that 0.78 mole of NH3is present. The reaction is2 NH3(g) 3 H2(g) + N2(g)(a) What is the number of moles of H2 and N2 at equilibrium?(b)What is the concentration in moles/liter of each component? Ans. (a) H
2 BrCl(g) Cl2(g)+ Br2(g)At a certain temperature the equilibrium constant for the reaction is 11.1, and the equilibrium mixture contains 4 mol Cl2. How many moles of Br2and BrCl are presentin the equilibrium mixture? 7. The decomposition of hydrogen iodide at 450oC produces an equilibrium mixture that contains 0.50 mol of hydrogen. The equilibrium constant is 0.020 for the reaction. How many moles of iodine and hydrogen iodide are present in the equilibrium mixture?