The following reaction establishes equilibrium at 2000K: N2(g) + O2(g) 2NO(g) where Keq - 4.1 x...
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
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?
Question 10 5 pts The value of the equilibrium constant for the reaction, N2(e)+0,6)=2NO(g), is 4.1 x 10-. Find the concentration of NO(g) in an equilibrium mixture with air at 1 atm pressure at this temperature. Ininitially.IN2] -0.036 mol/L and (0,10.0089 mol/L You may use the Module 3 File Upload to show your work or type as much as you can here. If you use the Module 3 File Upload, be sure to upload your file within 15 minutes of...
6. What changes in the equilibrium composition of the reaction: N2(g) + O2 (0) 2 2NO (0) will occur at constant temperature if : (a) the pressure (or concentration) of Nz () is increased? (b) the pressure (or concentration) of NO (g) is increased? (c) the total pressure of the system is increased? (d) the total volume of the system is increased? (e) add a catalyst? (f) decrease the concentration of O2(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?
Question 29 (1 point) Consider the decomposition reaction 2NO(g) + N2(g) + O2(g). When 0.20 M sample of NO(g) was decomposed at a given temperature, the equilibrium concentration of N2 was 0.040 M. What was the equilibrium concentration of NO(g)? 0.12 M 0.040 M 0.24 M 0.080 M Previous Page Next Page Page 29 of 30
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 reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture starts with only the product, [NO] = 0.0300 M , and no reactants. Part A Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the appropriate units. [N2] = Part B Find the equilibrium concentrations of O2 at equilibrium. Part C Find the equilibrium concentrations of NO at equilibrium. Express your answer to two significant figures...