Identify the proper form of the equilibrium-constant expression for the equation
N2(g)+O2(g)⇌2NO(g)
Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g)
Consider the reaction N2(g)+O2(g)↽−−⇀2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) that has an equilibrium constant, ?cKc, fof 4.10×10−44.10×10−4 at 17001700 °C. What percentage of O2O2 will react to form NO if 0.4850.485 mol N2N2and 0.4850.485 mol O2O2 are added to a 0.6870.687 L container and allowed to come to equilbrium at 17001700 °C?
atch each chemical equation below with the correct equilibrium constant expression Chemical Equation Equilibrium Constant Expression [Na][2] [N202] (N2)[02] (NO) K 2NO(g) = N2(g) +0:(0) [NZ][0212 [NO1 [N][0] [N,021 K- N2(g) + O2(g) + N20 (9) [NO] [NO] [N, (021 [N] [0,1 K- 2NO(g) = N219) + 20 (9) INO,] {N_02] [N][0,1 [N,10,1 KE N2(g) +20,(9) = 2NO,(9) [NO] IN] [O] IN][0]? [NO] N (9) +0,(g) = 2NO(g) [N, 021 IN] [0,1 INO, [N]?[0] K = N,0.(g) = N(g) +...
Which of the following is the equilibrium constant expression for the reaction: 2NO(g) + O2(g) - 2NO2(8) [NO] A. Kod [NO] [02] [no] [NO] [02] [NO] [NOJ +[02] 2[NO] D. K. INO]+[02] E. None of the choices are correct. Option A Option B
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.26, 0.36, and 0.030 atm, respectively, at 2200°C, what is KP?
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.20, 0.35, and 0.030 atm, respectively, at 2200° C, what is KP?
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g) Kc = 4.3 × 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: N2(g) + 2O2(g) ⇌ 2NO2(g)
Consider the following equilibrium system. N2(g) + O2(g) ⇌ 2NO(g) a) Write the chemical equation for the forward reaction. (Use the lowest possible coefficients. Use the smaller blank lines to specify states such as (aq) or (s). If a state is not needed, leave it blank. ___________ ___ + ___________ ___ -----------> ___________ ___ b) Write the chemical equation for the reverse reaction. (Use the lowest possible coefficients. Use the smaller blank lines to specify states such as (aq) or...
QUESTION 1 ins 2NO(g) ==== [CLO-5] Consider the following equilibrium the reaction: N2(g) + O2 (g). The initial concentration of NO is 0.175 M. Solving the quadratic equation yields two solutions for (x): x1 = 0.1292 and x2 = 0.0661. Selecting the correct root, what are the equilibrium concentrations of NO, N2 and O2? 0.175, 0.0661 0.0661 0.175, 0.1322 0.1322 0.0428, 0.0661, 0.0661 0.1089, 0.0661, 0.0661
QUESTION 12 BEE [CLO-6] At 2000 °C, the equilibrium constant for the reaction: 2NO(g) N2(g) + O2(g) Is Kc = 2.4. Knowing that the initial concentration of NO is 0.175 M, what will be the concentrations of NO, N2 and O2 at equilibrium? [Hint: you have to build a table to find the answer) (0.175), +2x, +2x (0.175), +x, +x +x (0.175-2x), +x, (0.175-x), +x, +X