The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O2 (g) What is the value of Kp at this same temperature? K = 1.7 x 1026 at 40,0°C (A) (B) (C) 4.4 x 10-25 6.6 x 1028 5.2 x 107 (D) 6.5 x 1030 (E) 5.9 x 1025

When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H2O(g) <--> CO2(g) + H2(g) +heat  For each of the following changes at equilibrium, indicate whether the equilbrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) (d) adding more H2O(g) (e) decreasing the volume of the container

2) For the reaction, PCI:(g) = PCl:(g) + Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol) (a) What would be the pressure of PCIs if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIS at cquilibrium?

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(b) At 100° C, the Keq for the Haber process is 4,51 X 10-5: N₂ + 3 H₂ 2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium (i) PNH3 105 atm, PN2 = 35 atm and PH2 = 495 atm (ii) PNH3 35 atm, PN2 = 0 atm and PH2 = 595 atm (iii) PNH3 = 26 atm, PN2 = 202 atm and PH2 = 42 atm (iv) PNH3 105 atm, PN2 = 5 atm and PH2 = 55 atm

For the reaction: H2 (g)+ Br2 (g)= 2 HBr(g) 104 Кр — 3.5 х 1495 K. at What is the value of Kp for each of the following reactions at 1495 K? (a) 2 HBr(g) - H2 (g)+ Br2 (g) Кр (b) H2 (g) + Br2 (g) = HBr(g) K, (c) HBr(g) = H2 (g) + Br2 (g) Kp =

The reaction N204(s) * 2NO2(3) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.183 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of N02 = atm (b) What was the total pressure of the mixture of gases? total pressure = atm