Kc is defined as concentration of product by concentration of reactant with each concentration term raised to power that is equal to its stoichiometric coefficient in balanced equation
so,
K = [NO]^2 / [N2][O2]
= (0.00956)^2 / (0.520 * 0.0662)
= 0.00265
Answer: 0.00265
Consider the reaction: N2(g) + O2 ) the value of K? 2 NO ) İf [N1-o520...
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...
Consider the following reaction. N2(g) + O2(g) 2 NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm, and 0.050 atm, respectively, at 2200°C, what is KP?
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 279 K 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 6.503×10-62 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 4.122×104
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?
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 291 K given the following information, 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 5.397×10-61 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 2.432×104
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated, carbon reacts with water to produce carbon monoxide and hydrogen. C(s)+H2O(g)+heat⇌CO(g)+H2(g) Part C What effect does each of the following changes have on the equilibrium? Drag the appropriate stresses to their respective bins. add H2O, Add heat, lower temperature, remove CO Categories: Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift
At equilibrium, the concentrations of N2(g), O2 (g) and NO (g) in a sealed reaction vessel are [N2]= 3.174x10-3 M, [O2]= 6.502x10-3 M, [NO]=2.563x10-3 M. What is the value of Kcfor the reaction? N2 (g) + O2 (g) ---> <---- 2NO (g)
The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is burned in air at a high temperature, as in a gasoline engine. At 1500 K, Kc = 1.0×10-3. Suppose a sample of air has [N2] = 0.70 mol/L and [O2] = 0.20 mol/L before any reaction occurs. Calculate the equilibrium concentrations of reactants and products after the mixture has been heated to 1500 K. [N2] = M [O2] = M [NO] = M
14.49. If the equilibrium constant K, for the reaction N2(g) + O2(g) – 2 NO(g) is 1.5 X 10%, in which direction will the reaction proceed if the partial pressures of the three gases are all 1.00 X 10-3 atm?