1.) The equilibrium constant for the chemical equationN2(g) 3H2(g) <--> 2NH3(g)is Kp = 1.09 at 209 °C. Calculate the value of the Kc for the reaction at 209 °C.2.) At a certain temperature 0.3411 mol of N2 and 1.581 mol of H2 are placed in a 1.50-L container.N2(g) 3H2(g) <--> 2NH3(g)At equilibrium 0.1801 mol of N2 is present. Calculate the equilibrium constant Kc.3.) At a certain temperature the Kp for the decomposition of H2S is 0.748.H2S(g) <--> H2(g) S(g)Initially only H2S is present at a pressure of 0.189 atm in a closed container. What is the total pressure in the container at equilibrium?4.) An equilibrium mixture contains 0.600 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container.CO(g) H2O(g) <--> CO2(g) H2(g)How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?5.) Write the equilibrium constant expression for the reaction below (Keq):CH4(g) 2H2S(g) <--> CS2(g) 4H2(g)A reaction mixture initially contains 0.50M CH4 ad 0.75M H2S. If the equilibrium concentration of H2 is 0.44M find the equilibrium constant (Kc) for the reaction.6.) Express the equilibrium constant for the following reaction.P4(s) 5O2(g) <--> P4O10(s)
