Consider the equilibrium system: 2 NOB (g) = 2 NO (g) + Br2 (g) At a 298 °K, analysis of an equilibrium mixture finds the following concentrations: [Br2] = 4.0 mol/L, [NOB1] = 0.50 mol/L, [NO] = 2.0 mol/L. Calculate Keg for the reaction at this temperature. %3D

Calculate the pressure of N2 needed to reverse the reaction (last row of the table. 0.38 is wrong). thank you!

Consider the following equilibrium: N2 (g) + 3H, (g) – 2NH; (g) AG = - 34. kJ Now suppose a reaction vessel is filled with 7.31 atm of nitrogen (N,) and 7.58 atm of ammonia (NH,) at 1074. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that yes be changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding H,? 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. O O

The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K.2SO3(g) 2SO2(g) + O2(g)If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1030 K?Kp =  ---   The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K.PCl3(g) + Cl2(g) PCl5(g)If ΔH° for this reaction is -87.9 kJ, what is the value of Kp at 416 K?Kp =

Consider the following system at equilibrium where H° = -198 kJ/mol, and Kc = 34.5 , at 1150 K.2 SO2 (g) + O2 (g)  2 SO3 (g)When 0.10 moles of SO3 (g) are added to the equilibrium system at constant temperature:The value of Kc    The value of Qc     Kc.The reaction must run in the forward direction to restablish equilibrium.run in the reverse direction to restablish equilibrium.remain the same.  It is already at equilibrium. The concentration of O2 will

32 Consider the reaction: kJ 2SO₂(g) + O₂(g) =2SO3(g) AH= - 198.2 mol How would the concentrations of SO2, O₂, and SO3 at equilibrium change if we were to increase the temperature? Select the single best answer for each part. Part 1 of 3 [s0₂]: The concentration increases. [0₂]: The concentration decreases. There is no change. Part 2 of 3 The concentration increases. The concentration decreases. There is no change. X X S

Consider the reaction: CO(g) + Cl₂(g) COC12 (g) € Kp At equilibrium, this reaction is At equilibrium, the rates of→ and reaction are equal. At equilibrium, reactant and product concentrations are constant. Reactions continue after equilibrium has been reached. Decreasing the temperature changes the K, value for this reaction. Removing COC1₂(g) changes the value of K, for this reaction. For the reaction: COCI, (g) = CO(g) + Cl₂(g), the value of K, is equal to 6.7 x 10¹1 at 25°C V V

Choose the letter of the correct answer. N204 (g) = (reversible to) 2NO2 (g), K = 4.63 x 10-3 I. the given is equation is an example of homogenous equilibrium II. Equilibrium will lie to the right Which statement(s) is/are correct?

The synthesis of CaCO3 uses this chemical reaction. CaO(aq) + CO2(g) ——> CaCO3(s) + 180 kJ Identify three stresses that can be imposed on the equilibrium to maximize the amount of CaCO3 present. Be specific about what, if any, compounds are involved in those stresses.

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