) The equilibrium constant Keq= 1.85 x 10-6 for the reaction: A(g) +3B(g) ⇌2C (g) Calculate: ΔGo       Q and ΔG for the same reaction under the following nonstandard conditions: [A] = 2 M ; [B] = 7 M ; [C] = 0.021 M ; Temperature = 100oC.

The Kp for 3A(g) + 4B(g) = 2C(g) + 3D(s) is 4.90 x 10-4 at 300C. Determine the Kc for this reaction at the same temperature.

1) Given the following reaction at 298K: 2POF3(g) ⇌ 2PF3(g)+O2(g) ΔG°rxn=+537.8 kJ/mole A) Calculate the value for K. B) When the reaction reaches equilibrium, rank the species (POF3, PF3 and O2) in order from least to greatestconcentration.

Consider the following reaction at 298 K:N2 O4(g) ⇌ 2NO2(g)              KP = 0.142What is the standard free energy change at this temperature? Describe what happens to the initial system, where the reactants and products are in standard states, as it approaches equilibrium.

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: 2NO, (g) – N,04(g) AG = - 5.4 kJ Now suppose a reaction vessel is filled with 7.26 atm of dinitrogen tetroxide (N,O) at 95. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can that yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,0, will tend to fall, can that be changed to a tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it. atm Round your answer to 2 significant digits. O O

In which of the following reactions is ASº expected to be negative? O L(s)I(g) O 2NH;(g) → N(g) + 3H3(g) O 2H,0(g) → 2H,(g) + O>(g) O CH;OH(g) → CH;OH(I) O AS° is not expected to be negative for any of these.

Predict the change in the preturbations table below. Also decide whether the equilibrium shifts to the right or left.

We start with a sample of pure A(g). The following equilibrium is established 2 A(g) <---> B(g) + C(g) The total pressure is 8.33 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.26 atm. Calculate the value of the standard free enthalpy change (in kJ) of this reaction at 25.0oC.

The equilibrium constant, Kċ, for the following reaction is 1.29×10-² at 600 K. Calculate Kp for this reaction at this temperature. COCI₂(g) ⇒CO(g) + Cl₂(9) Кр || =