Calculate the value of the equilibrium constant for the reaction, 4NH3(g)+3O2(g)⇌2N2(g)+6H2O(g) given the following equilibrium constants at a certain temper

Consider the reaction: N₂ (9) +202 (g) ⇒ N₂O4 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N₂O4 (9) 2NO₂(g) K₁ 1/2N₂(g) + O₂(g) NO₂ (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K =

The equilibrium constant for the reaction 2 HF (g) ⇌ H₂ (g) + F₂ (g) is 0.300 at a particular temperature. What is the equilibrium constant for the equation ½ H₂ (g) + ½ F₂ (g) ⇌ HF (g)?

For the reaction N2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g) KpKpK_p = 4.25×10−3 at 334 ∘C∘C . What is KcKc for the reaction at this temperature? Enter your answer numerically.

10:01 1 Question 3 of 25 Submit Consider the equilibrium constant below. Which of the following reactions would fit this equilibrium constant? Кр P. P3 D A) C (g) + 3 D (g) =2 A (g) + B (g) B) 2 A (g) + B (g) =C (g) + 3D (g) C) A (g) + B (g) =C (g) + D (g) D) C (g) + D (g) = A (g) + B (g)

As shown in Table 15.2 in the textbook, KpKp for the equilibriumN2(g)+3H2(g)⇌2NH3(g)N2(g)+3H2(g)⇌2NH3(g)is 4.51×10−54.51×10−5 at 450 ∘C∘C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 ∘C∘C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. A. 98 atmatm NH3NH3, 45 atmatm N2N2, 55 atmatm H2H2 98  , 45  , 55   a. yes, mixture is at equilibrium b. no, mixture must shift toward products to achieve equilibrium c. no, mixture must shift toward reactants to achieve equilibrium B.57 atmatm NH3NH3, 143 atmatm N2N2, no H2H2 57  , 143  , no  a.yes, mixture is at equilibrium b.no, mixture must shift toward products to achieve equilibrium c.no, mixture must shift toward reactants to achieve equilibrium

Initially, 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter container and the reaction below then occurred. The equilibrium concentration of NH3(g) = 0.55 M at 700.°C. The value for Kc at 700.°C for the formation of ammonia is: 3H2(g) + N2(g) ⇌ 2NH3(g) a) 1.0 x 10^-1 b) 5.5 x 10^-2 c) 5.5 x 10^-3 d) 3.0 x 10^-1 e) The correct answer was not initially available

The following reactions have the indicated equilibrium constants at a particular temperature:  N2 (g) + O2(g) ⇌ 2NO (g) Kc = 7.1 ×10−25 2NO (g) + O2 (g) ⇌ 2NO2(g) Kc = 6.4 × 109 Determine the value of the equilibrium constant for the following equation at the same temperature:  2NO(g) ⇌ N2(g) + O2(g)

Consider the following reaction at equilibrium at 400 K: 2SO2(g) + O2(g)  ⇌  2SO3(g)                      K = 15.0 If the partial pressures of SO2(g) and O2(g) are 0.23 atm and 0.35 atm, respectively, then what is the partial pressure of SO3(g)?

Consider the equilibrium system below, 2C2H6(g)   +   7O2(g)   ⇌   4CO2(g)   +   6H2O(g)         ∆H = -3120 kJ How will the amount of ethane (C2H6) at equilibrium be affected by: decreasing the temperature? decrease, increase, no effect decreasing the volume of the container at constant temperature? decrease, increase, no effect