Consider the following system at equilibrium where AH° = 198 kJ, and K. 2.90x102, at 1150 K: %3D 2S03(g)2S02(g) + O2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of K. A. Increases B. Decreases C. Remains the same

For the first one the options are increases, decreases, and remains the same.

Consider the following equilibrium: 2NH, (g) – N, (g) + 3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 5.02 atm of ammonia (NH,) and 9.40 atm of nitrogen (N,) at 159. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N, tend to rise or fall? fall Is it possible to reverse this tendency adding H2? In other words, if you said the pressure of N, will tend to rise, can that be yes changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of N, will tend to fall, can that be changed to a tendency to rise by adding H2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. atm Round your answer to 2 significant digits.

Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S