At 1000 K, the Kc values of the following reactions are:1) N2O4(g) ⇌ 2NO2(g) Kc = 1.5x1062) N2(g) + 2O2(g) ⇌ 2NO2(g) Kc = 1.4x10-10What is the Kc of the following reaction at 1000K? N2(g) + 2O2(g) ⇌ N2O4(g)

The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?

Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.

Answer the following questions regarding the butane isobutane equilibrium (Kc = 2.50 at 298 K). (a) Is the system at equilibrium when [butane] = 0.00097 M and [isobutane] = 0.00218 M? If not, in which direction will the reaction proceed to achieve equilibrium? (b) Is the system at equilibrium when[butane] = 0.00075 M and [isobutane] = 0.00260M? If not, in which direction will the reaction proceed to achieve equilibrium?

Consider the following system at equilibrium at 25C: PCl3(g)+Cl(g)PCl5(g)G=92.50KJ What will happen to the ratio of partial pressure of PCl5 to partial pressure of PCI3 if the temperature is raised? Explain completely.

Carbon dioxide decomposes into CO and O2 at elevated temperatures. What is the equilibrium partial pressure of oxygen in a sample at 1000 C for which the initial pressure of CO2 was 1.15 atm?

Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g) At a certain temperature, the equilibrium partial pressures of SO2, Cl2, and SO2Cl2 are 1.88 atm, 0.84 atm, and 0.27 atm, respectively. (a) What is K at that temperature? (b) Enough Cl2 condenses to reduce its partial pressure to 0.68 atm. What are the partial pressures of all gases when equilibrium is reestablished?

Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?

Consider the following relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these relationships is(are) always true for a reaction at equilibrium?

Consider the following hypothetical reactions and their equilibrium constants at 75C, 3A(g)3B(g)+2C(g)K1=0.31 3D(g)+2B(g)2C(g)K1=2.8 Find the equilibrium constant at 75C for the following reaction A(g)D(g)+53B(g)