5. The decomposition of nitrogen dioxide is a second order reaction with rate constants as follows:...
The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 9.17 ×10-3 s-1. Starting with pure N2O4, how many minutes will it take for 85.0% to decompose?
QUESTION 22 The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 9.17 X10sl. Starting with pure N204, how many minutes will it take for 85.0% to decompose? *Please report 3 significant figures. Numbers only, No unit. No scientific notation.
The rate constant for the decomposition of nitrogen dioxide NO2(g) LaTeX: \longrightarrow ⟶ NO (g) + 1/2 O2(g) with a laser beam is 1.76 1/MLaTeX: \cdot ⋅ min. Find the time, in seconds, needed to decrease 2.4 M of NO2 to 1.18 M. Hint: What is the order of the reaction? How can you determine that? Units of k?
1) 2) 3) The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 3.84 X10-3-1. Starting with pure N204, how many minutes will it take for 38.0% to decompose? Suppose the surface-catalyzed hydrogenation reaction of an unsaturated hydrocarbon has a rate constant of 0.374 M/min. The reaction is observed to follow zero-order kinetics. If the initial concentration of the hydrocarbon is 2.90 M, what is the half-life of the reaction in seconds?...
At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: The reaction is second order in NO2 with a rate constant of 0.543 M-1 s-1 at 300°C If the initial [NO2] is 0.260 M it will take ________ seconds for the concentration to drop to 0.100 M. 11.3 8.8 × 10-2 -0.611 3.34 0.299
The reversible gas-phase decomposition of nitrogen tetra oxide, N2O4, to nitrogen dioxide, NO2, is to be carried out at constant temperature. The feed consists of pure N2O4 at 340 K and 202.6 kPa (2 atm). The rate constant of forward reaction is 0.5 min-1 and the equilibrium constant, Kc, at 340 K = 0.1 mol/dm3. N2O4 2NO2 Use POLYMATH, calculate the equilibrium conversion of N2O4 in a flow reactor. We were unable to transcribe this imageWe were unable to transcribe...
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of N2O4 became 2 times less after 2,5⋅103 s. You have to calculate: a) the value of rate constant k of the reaction; b) the value of equilibrium constant Kp. You are given the value of standard Gibb’s energy of formation Goform: substance Goform, kJ/mol NO2(g) 51.6 N2O4(g) 98.4
The decomposition of nitrogen dioxide occurs according to the equation below: NO2 (g)------>NO( g)+1/2 O2 (g) The reaction is second order with respect to NO2. The specific rate constant for this reaction is 3.04M-1min-1. How long does it take for the concentration of NO2 to decrease from 2.00M to 1.25M?
The decomposition of nitrogen dioxide at a high temperature NO_2(g) rightarrow NO(g) + 1/2 O_2(g) is second-order in this reactant. The rate constant for this reaction is 3.40 L/mol min. Determine the time needed for the concentration of NO_2 to decrease from 2.00 mol/L to 1.50 mol/L.
Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction: N2O4(g) → 2NO2(g) At 400.0 K, the rate constant for this reaction has been measured to be 2.9 × 108 L/(mol • s). Suppose 0.222 mol of N2O4(g) is placed in a sealed 41.7-L container at 400.0 K and allowed to react. What is the total pressure inside the vessel after 32.9 ns has elapsed? (R = 0.0821 (L • atm)/(K • mol)) a. 0.183 atm b. 0.175 atm...