A sample of NO decomposes according to the following equation: 2 NO(g)  1 N2(g) + 1 O2(g) An equilibrium mixture in a 3-L vessel at 4497 oC, contains 0.000759 g of NO, 0.00202 g of N2, and 0.00138 g of O2. (a) Calculate KP for this reaction at this temperature. (b) What is the total pressure exerted by the equilibrium mixture of gases?

At 25°C, the equilibrium constant for the reaction Blg) + Clg) 2A(3) is K,-0.0735.If the three gases are mixed in a rigid container having partial pressuros of 3.35, 185 and 0.693 atm for A, B and C, respectively, is the system at equilibrium? The system is at equilibrium. The reverse reaction must proceed to establish equilibrium. The volume of the container must be known to answer the question. The concentrations of all substances must be known to answer the question. The forward reaction must praceed to establish equilibrium,

A flask is charged with 1.500 atm of N2O4(g) and 1.00 atmNO2(g) at 25 °C, and the following equilibrium is achieved:N2O4(g) ⇌ 2 NO2(g)After equilibrium is reached, the partial pressure of NO2is 0.512 atm. (a) What is the equilibrium partial pressureof N2O4? (b) Calculate the value of Kp for the reaction.(c) Calculate Kc for the reaction.

The reaction N₂O4(g) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4 was 0.287 atm. (a) What was the partial pressure of NO₂ in the reaction mixture? pressure of NO₂ = atm (b) What was the total pressure of the mixture of gases? total pressure = i atm

Phosphorous pentachloride decomposes at 600. °C according to the following equation. PCI, = PCl (g) + Cl,(g) After the system comes to equilibrium the partial pressures of both Cl and PCl; are found to be 3.14 atm, and the partial pressure of PCI5 was 0.858 atm. Calculate K (not Kp) for this reaction at 600 °C.

5. The Water Gas equilibrium, co (8) + H20 (g) = CO2 (g) + H2 (g) has a equilibrium position when the pressure of CO, H2O, CO2 and H2 are, respectively, 0.500 atm, 1.00 atm, 0.167 atm and 3.00 atm at 1100 K. (a) What is the value of Kp at 1100 K? (b) Is the system at 1100 K at an equilibrium position when the respective pressures are 1.00 atm, 2.00 atm, 0.334 atm and 6.00 atm? If not, then in which direction will the system shift?

(5b) Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 )2 as (P NH3)2. If either the numerator or denominator is 1, please enter 1   2 CuCl2(s)   ↔   2 CuCl(s) + Cl2(g)           K   =     (8c) Consider the following reaction where Kc = 6.50×10-3 at 298 K: 2 NOBr (g) 2 NO (g) + Br2 (g) A reaction mixture was found to contain 9.96×10-2 moles of NOBr (g), 4.61×10-2 moles of NO (g), and 4.42×10-2 moles of Br2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed .2. In order to reach equilibrium Kc must decrease .3. In order to reach equilibrium NO must be produced .4. Qc is less than Kc.5. The reaction is at equilibrium. No further reaction will occur.

What is the value of Kp at 675.00 K?

Consider the reaction N2(g) + O2(g) = 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.28, 0.26, and 0.025 atm, respectively, at 2200°C, what is Kp?

The reaction N₂O4(g) 2NO₂(g) has a Kp = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N₂O4 was 0.344 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO₂ = atm (b) What was the total pressure of the mixture of gases? total pressure = atm