12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) +...

Question

Question

Answer 1

Answer #1

+ 2NH3 (9) . N2 (9) + 3H2(g) ke- (Paris) ra) (P) (P) TM (s) + 34,6) 2014 2 15) 160-y 1.4-34 (24)2 kp= (-y) (4-3y)3 4.51x105.

Answer 2

Similar Homework Help Questions

The equilibrium constant, Kp, is 4.51 x 10-35 at 450c for the reaction expressed below. N2...

The equilibrium constant, Kp, is 4.51 x 10-35 at 450c for the reaction expressed below. N2 (g) + 3H2 (g) equilibrium arrows 2 NH3 (g) a. Write the equilibrium expression for, Kp, for the reaction. b. Supposed you start out with only reactants in a rigid container. The initial partial pressure of N2 (g) is 1 atm and that of H2 is 1.4 atm. What ate the partial pressure of each species when the system reaches equilibrium? Can you explain...
For the reaction represented below, the value of the equilibrium constant, Kp is 3.1 × 10-4...

For the reaction represented below, the value of the equilibrium constant, Kp is 3.1 × 10-4 at 700 K. N2 (g) + 3H2 (g) ⇌ 2NH3 (g) Assume that the initial partial pressures of the gases are as follows: P(N2) = 0.411 atm, P(H2) = 0.903 atm, and P(NH3) = 0.224 atm. Which of the following is true? Q < K Q > K Q = K
3. {7} Consider equilibrium N2 (g) + 3 H2(g) 5 2NH3(g) K, -4,51 x10-at 450 °C....

3. {7} Consider equilibrium N2 (g) + 3 H2(g) 5 2NH3(g) K, -4,51 x10-at 450 °C. For the mixture below indicate the direction of this equilibrium reaction toward product or toward reactants) at the following partial pressures: 105 atm NH3; 35 atm N2; 495 atm H:

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400...

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...
At 7075 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + 02(9) is Kp...

At 7075 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + 02(9) is Kp 0.983. If the initial pressure of NO is 0.00863 atm, what are the equilibrium partial pressures of NO, N2, and O2? P(NO) P(N2) p(02)
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches...

At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10−2 atm, respectively. Given that the standard enthalpy of the reaction at 400K is DH = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature...

1/2 N2 (g) +3/2H2 (g) ⇌ NH3 (g) a) Given t=450 C p= 40 atm and...

1/2 N2 (g) +3/2H2 (g) ⇌ NH3 (g) a) Given t=450 C p= 40 atm and Kp= 7x10^-3 atm^-1 what is Kc? b) If the gases are placed in a closed reaction vessel with the partial pressures PNH3= 24 atm, PN2= 12 atm and PH2= 36 atm is the system in equilibrium? c) If the vessel is allowed to expand such that the total pressure is 10 atm will H2 (g) form or be consumed? d) If the temp is...
At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP...

At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 7.16. If the initial pressure of NO is 0.00663 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .
N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined...

N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined using atm) A 7.5 x 101 L container being held at 298 K is charged with the three gases present in the above equation. Once finished, the initial partial pressure of N2 was 0.59 atm, the initial partial pressure of H2 was 0.45 atm, and the initial partial pressure of NH3 was 0.11 atm. The gas mixture was then allowed to reach equilibrium. Use...

The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g)...

The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.