1) Dinitrogen tetroxide partially decomposes according to the following equilibrium : N204 (9) = 2'N02 (9)....
I NEED HELP WITH THIS PROBLEM SOMEONE HELP PLEASE!!! Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204(g) → 2NO2(g) A 1.000-L flask is charged with 2.60 x 10-2 mol of N204. At equilibrium, 2.01 x 10 2 mol of N204 remains. Keg for this reaction is O 0.361 O 1.53 x 10-4 O 0.615 6.94 x 10-3
Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4(g) 2NO2(g) A 1.000 L flask is charged with 6.00 × 10-2 mol of N2O4. At equilibrium, 3.21 × 10-2 mol of N2O4 remains. Kc for this reaction is ________. Group of answer choices 0.465 2.42 × 10-2 1.74 10.3 9.70 × 10-2
Dinitrogen tetroxide decomposes to produce nitrogen dioxide: N204 (9) - 2 NO2 (g) Calculate the equilibrium constant for the reaction given the equilibrium concentrations at 100°C: [N204] = 0.800 M and [NO2] = 0.400 M A. 5.00 OB.0.200 OC. 0.500 OD.2.00
When heated, colorless dinitrogen tetraoxide, N204(8), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204(g) 42 NO2 (g) Suppose that 2.00 mol of N204(8) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K., for this reaction at 407 K. 0.500 O 0.525 2.00 0.263 3.80
2. For the equilibrium between dinitrogen tetroxide and nitrogen dioxide: N204 = 2 NO2 Suppose that both the forward and reverse reactions are elementary processes with rate constants of k, and kr respectively, and the equilibrium constant for the process is 14.48 at 298 K. If the rate of the reverse reaction is 1324 M/s when (NO2) = 0.60 M, what is the half-life for the decomposition of dinitrogen tetroxide (the forward reaction) at the same temperature?
When heated, colorless dinitrogen tetraoxide, N2O4(g), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204 (g) + 2 NO2 (g) Suppose that 2.00 mol of N204(g) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K, for this reaction at 407 K. 3.80 2.00 0.500 0.263 0.525
For the dimerization of nitrogen dioxide to form dinitrogen tetroxide (N2Oa) according to the reaction 2 NO,()-N,0,) [the sign is intended to be an equilibrium arrow), the value of AH° is-57.2 kJ/mol, and that of AS is-175.8 J/ (mol K). Estimate AG° at 100.0 °C. +6.6 kJ/mol -39.6 kJ/mol -122.8 kJ/mol -74.8 kJ/mol O+8.4kJ/mol
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains 0.100 bar of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 369 K? Assume that the initial pressure of N2O4 is the same (0.100 bar)
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains 0.100 bar of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 389 K? Assume that the initial pressure of N2O4 is the same (0.100 bar). Please use bar and not atm.
1) 2) 3) At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 IC1(g)=12(8) + Cl2(g). What is the equilibrium concentration of Cl2 if 3.18 mol of I2 and 3.18 mol of Cl2 are initially mixed in a 2.0-L flask? The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 2.86 x10-35-1. Starting with pure N204, how many minutes will it take for 80.0% to decompose? *Please report...