The equilibrium constant expression K p for the reaction 2NH 3 (g) ↔ N2 (g) + 3H2 (g) is __________.
A. Kp = PN2(3PH2)3/(2PNH3)2
B. Kp = PNH32/PN2PH23
C. Kp = (2PNH3)2/PN2(3PH2)3
D. Kp = PN2PH23/PNH32
If the solution helps then rate it.
The equilibrium constant expression K p for the reaction 2NH 3 (g) ↔ N2 (g) + 3H2 (g) is __________. A. Kp = PN2(3PH2)3/...
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...
The equilibrium constant expression K p for the reaction CH4 (g) +2O2 (g) <--> CO2 (g) + 2H2O (g) is __________. A. Kp = PCO2PH2O 2/PCH4PO22 B. Kp = PCH4PO22/PCO2PH2O 2 C. Kp = PCH4PO2/PCO2PH2O D. Kp = PCO2PH2O /PCH4PO2
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 PCl3(g) + Cl2(g) ↔ PCl5(g) K = 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,...
The equilibrium constant expression K p for the reaction O2 (g) + H2 (g) <--> 2H2O (g) is __________. A. Kp = PH2O2/PO2PH22 B. Kp = PO2PH22/PH2O2 C. Kp = PH2O/PO2PH2 D. Kp = PO2PH2/PH2O
For: N2(g) + 3H2(g) ⬄ 2NH3(g), Kp = 4.72 x 10–4 at 475 oC. At equilibrium at 475 oC, PH2 = 0.237 atm and PN2 = 0.582 atm. What is the partial pressure of ammonia at equilibrium?
12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) + 3 H2(g) 2 NH3(g) a. Write the equilibrium expression, Kp, for the reaction. b.Suppose y ou start out with only reactants in a rigid container. The initial partial pressure of N2(g) is 1.0 atm and that of H2(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium? c. Find K, for this process at 450°C.
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 value of the Kc for the reaction at 273 °C.
KP = 1.000 x 10–4 for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). The reaction is at equilibrium when PH2 = 4.00 atm, PN2 = 4.00 atm, and PNH3 = 0.16 atm. a) Show that these are equilibrium concentrations. b) If the pressure of the system is doubled (the pressure of each gas doubles), what is the final pressure of each gas when equilibrium is restored? If making and using ammonia is important to feeding the world's growing population but...
For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp = 3.50×10−3 at 262 ∘C . What is K for the reaction at this temperature?