please answer ALL questions & show all work!! thank you!

- 1. At a particular K = 3.75 for the reaction SO,(9) + NO,(9) 50,(9) + NO(g) If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of all of the gases. 2. At 25C, K = 0.090 for the reaction H.0(9) + C1,0(9) =2HOCK(9) Calculate the concentration of all species at equilibrium when 1.0 g H,0 and 2.0 g C1,0 are mixed in a 1.0 L flask. 3. A sample of S. (9) is placed in a an empty rigid container at 1325K at an initial pressure of 1.00 atm, where it decomposes to S. (9) by the reaction S.(9) 45,(9) At equilibrium, the partial pressure of s, is 0.25 atm. Calculate K, for this reaction at 1325K. 4. For the reaction described by the equation N. (9) + CH (9) 2HCN(9). K. = 2.3 x 10+ at 300C. What is the equilibrium concentration of HCN if the initial concentrations of N, and CH, were 3.5 M and 2.5 M, respectively? For #5 & #6 just set-up the equilibrium expression in terms of x...but do not solve for x. 5. At 35C, K. = 1.6 x 10" for the reaction, 2NOCI(9) 2NO(9) + C,(9). Calculate the concentrations of all species at equilibrium for 2.0 mole of NOCI in a 2.0 L. 6. The equilibrium constant, K, for the reaction N. (9) + 3H2(g) + 2NH,(9) at 450C is 0.159. Calculate the equilibrium composition when 1.00 mole N, is mixed with 3.00 mole H, in a 2.00 L container