Nitrosyl chloride, NOCl , decomposes to NO and Cl2 at high temperatures, as follows:   2 NOCl(g) ⇌ 2 NO(g) + Cl2(g)   Suppose you place 2.65 mol NOCl in a 1.00 L flask and raise the temperature to 462o C. When equilibrium has been established, 0.81 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.

A student ran the following reaction in the laboratory at 290 K:2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 8.37×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 6.14×10-3M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.366 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K

At a certain temperature, the equilibrium constant K for the following reaction is 0.0017: CO(g)+ H₂O(g) CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 27. L reaction vessel is filled with 1.5 mol of CO and 1.5 mol of H₂0. 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. CO,(9)+H,(9) CO(g)+H,O(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 CO(g) + 2H₂O(g) 2 CO₂(g)+2H₂(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