Question

Consider the following equilibrium: Now suppose a reaction vessel is filled with 8.04 atm of nitrogen monoxide (NO) and 9.09 atm of nitrosyl chloride (NOCI) at 1009. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NO tend to rise or fall? fall Is it possible to reverse this tendency by adding Cl2? In other words, if you said the pressure of NO will tend to rise, can that be changed to a tendency to fall by adding Cl2? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl2 If you said the tendency can be reversed in the second question, calculate the minimum pressure of C12 needed to reverse it Round your answer to 2 significant digits yes

Answer 1

In the beginning as there is no cl_2, the pressure of no increases because of backward reaction rightarrow rise rightarrow by adding cl_2 it is possible to reverse the process rightarrow yes rightarrow delta G degree = -RT ln K T = 1009 degree c = 1282.15K -41*10^3 = -8.314*1282.15 lnK K = 46.816 from equation: K = PNO^2cl/PN^2O * Pcl_2 46.816 = 9.09^2/8.04^2 x the minimum pressure of cl_2 required = pcl_2 = 0.0273 atm.