The equilibrium constant for the chemical equation N2(g) 3 H2(g)2NH3 (g) is Kp = 0.0146 at...

Question

Question

The equilibrium constant for the chemical equation N2(g) 3 H2(g)2NH3 (g) is Kp = 0.0146 at 183 oC. Calculate the value of Kc

science chemistry

Answer 1

Answer #1

C We know プhaう。 moles Here Ke 0146 0.0146 Kc (6.3/y x456 ). = Ko.olyb 2 3191.104) 2 ん O.Oly6x (3791,184)

Answer 2

Similar Homework Help Questions

The equilibrium constant for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is Kp=0.111 at 231 ∘C. Calculate the value...

The equilibrium constant for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is Kp=0.111 at 231 ∘C. Calculate the value of Kc for the reaction at 231 ∘C.
The equilibrium constant (Kp) for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is 0.0200 bar−2 at 273 °C. Calculate...

The equilibrium constant (Kp) for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is 0.0200 bar−2 at 273 °C. Calculate the value of the Kc for the reaction at 273 °C.
The equilibrium constant for the chemical equation N2 g) +3H 2(g) 근 2NH3(g) is Kp =...

The equilibrium constant for the chemical equation N2 g) +3H 2(g) 근 2NH3(g) is Kp = 71.7 at 177 °C. Calculate the value of the Ke for the reaction at 177 °C. Number K,= Tools x 102

The equilibrium constant for the chemical equation N,(g) + 3H2(8) - 2NH3(g) is Kp = 0.0881...

The equilibrium constant for the chemical equation N,(g) + 3H2(8) - 2NH3(g) is Kp = 0.0881 at 225 °C. Calculate the value of K, for the reaction at 225°C. Kc =
2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05....

2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05. What is the equilibrium constants Kc and Kp for the reaction 4NH3 + 2N2(g) + 6H2(g)? Kp = 400 Kc = 7.62 x 10 3. For the reaction given below, 10.00 moles of A and 25.00 moles of B are placed in a 5.00-L container at 120 °C. A(g) +2B(g) → C(g) At equilibrium, the concentration of A is 0.5 mol/L. What is the...
Write equilibrium constant expressions, Kp, for the following reactions. i) N2(g) + 3 H2(g) ⇌ 2NH3(g)...

Write equilibrium constant expressions, Kp, for the following reactions. i) N2(g) + 3 H2(g) ⇌ 2NH3(g) ii) NH4HS(s) ⇌ NH3(g) + H2S(g)

The equilibrium constant for the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g) is ?p=0.0752 at 221 ∘C. Calculate the value...

The equilibrium constant for the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g) is ?p=0.0752 at 221 ∘C. Calculate the value of ?c for the reaction at 221 ∘C.
A) For the Haber process, N2(g) + 3H2(g) <---> 2NH3(g), Kp = 4.34 x 10–3 at...

A) For the Haber process, N2(g) + 3H2(g) <---> 2NH3(g), Kp = 4.34 x 10–3 at 300oC. Pure NH3 is placed in a 2.00 L flask and is allowed to reach equilibrium at 300oC. There are 3.00 g NH3 in the equilibrium mixture. Calculate the mass (in g) of H2 in the equilibrium mixture. B) The value of Kc for the reaction is 1.2 . The reaction is started with [H2 ]0 = 0.76 M, [N2]0 = 0.60 M and...
Calculate the equilibrium equilibrium constant Kp for the reaction: N2 + 3H2 ↔ 2NH3, if the...

Calculate the equilibrium equilibrium constant Kp for the reaction: N2 + 3H2 ↔ 2NH3, if the partial pressures of N2, H2, and NH3 are 1.20 atm, 1.97 atm, and 0.225 atm respectively. A. 0.055 B. 0.532 C. 0.952 D. 18.2

3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2...

3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g) b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc c) Calculate the Kp for this reaction d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to nearly 100% completion? Explain f) If Qc...