Even at high temperatures, the formation of NO is not
favored:
(Kc = 4.10 ×10−4 at 2000°C)
N2(g) + O2(g) ⇌ 2
NO(g)
What is [NO] when a mixture of 0.20 mol of
N2(g) and 0.17 mol of O2(g)
reach equilibrium in a 1.0−L container at 2,000°C?
Even at high temperatures, the formation of NO is not favored: (Kc = 4.10 ×10−4 at 2000°C) N2(g) + O2(g) ⇌ 2 NO(g) What...
#17.10 Enter your answer in the provided box. Even at high temperatures, the formation of NO is not favored: (K = 4.10 x 10-4 at 2000°C) N2(g) + O2(g) = 2 NO(g) What is [NO] when a mixture of 0.20 mol of N2(g) and 0.17 mol of O2(g) reach equilibrium in a 1.0-L container at 2,000°C? M
apter 17 Homework Saved 1 attempts left Check my work Enter your answer in the provided box. Even at high temperatures, the formation of NO is not favored: (K. = 4.10 X 10 - at 2000°C) Hook N2(g) + O2(2) = 2 NO() nint rences What is [NO] when a mixture of 0.20 mol of N2(g) and 0.20 mol of O2(e) reach equilibrium in a 1.0-1 container at 2,000°C? Repc M Guld
Need help answering the questions with steps and explanation 1. even at a high temperature, the formation of NO is not favored. Compound A decomposes according to the equation A(g) 2 B(g)+ C (g) A sealed 1.00-L container initially contains 1.81 x 10 mol of A(g), 1.35 x 10 mol of B(g), and 6.58 x 10 mol of C(g) at 100°C. At equilibrium, [A] is 2.11 x 10 M. Find [B] and [C] Solve for the equilibrium concentrations of B...
1. A key step in the extraction of iron from its ore is FeO(s) + CO(g) ⇌ Fe(s) + CO2(g) Kp = 0.403 at 1,000°C This step occurs in the 700°C to 1,200°C zone within a blast furnace. What are the equilibrium partial pressures of CO(g) and CO2(g) when 1.1000 atm of CO(g) and excess FeO(s) react in a sealed container at 1000°C? 2. Compound A decomposes according to the equation A(g) ⇌ 2 B(g) + C (g) A...
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp =0.11 at 250°C NH HS(s) H2S() +NH3() If 60.5 g of NH HS(s) is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium? PN atm Enter your answer in the provided box. Even at high temperatures, the formation of NO is not favored: (K-4.10x 10 at 2000°C) N28)+O2(g)= 2 NO(g) What is (NO] when a...
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?
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
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L container, 1.0 mol of N2 and O2 are mixed. Determine the concentration of NO once equilibrium is reached at the given temperature. =________ Please explain so I understand
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of NO when the reaction mixture reaches equilibrium? Concentrations of NO= UNITS If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of N2 when the reaction mixture reaches equilibrium? Concentrations of O2= If the...
Ammonia can be oxidized in oxygen as shown: 4 NH3(g) + 3 O2(g) <=> 2 N2(g) + 6 H2O(g). When 0.541 mol of NH3 and 0.595 mol of O2 are placed in a 1.00 L container at a certain temperature, the equilibrium {N2} is 0.1347. Calculate the value of Kc for the reaction. Give your answer to 4 decimal places.