For a second order reaction,
1[A] = 1/[Ao] + kt
with,
[Ao] = 2.00 mol/L
[A] = 1.50 mol/L
k = 3.40 L/mol.min
t = time
we get,
1/1.5 = 1/2 + 3.40 x t
time needed for concentration of NO2 to decrease = 0.05 min
The decomposition of nitrogen dioxide at a high temperature NO_2(g) rightarrow NO(g) + 1/2 O_2(g) is...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
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Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g) + O_2(g) 2 NO_2(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M, O_2 is 0.100 M, and NO_2 is 0.250 M at 25 degree C? 8.00 times 10^-2 6.41 times 10^-2 12.5 15.6
The decomposition of NO2 at high temperature NO2(g) → NO(g) + 1/2 O2(g) is a second order process with a rate constant of 3.40 L/mol•min. If an experiment is performed where the initial concentration of NO2 is 0.400 M, what is the concentration of NO2after 2.96 min? [NO2] = M
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?
The reaction NO_2 (g) + NO (g) doublesidearrow N_2O (g) + O_2 (g) reached equilibrium at a certain high temperature. Originally, the reaction vessel contained the following initial concentrations: 0.184 M N_2O, 0.377 M O_2, 0.0560 M NO_2 and 0.294 M NO. The concentration of NO_2, the only colored gas in the mixture, was monitored by following the intensity of the color. At equilibrium, the NO_2 concentration had become 0.118 M. What is the value of Kc for the reaction...
The rate constant for the first-order decomposition of N_2O_5 in the xeactron2 N_2O_5(g) rightarroe 4 NO_2(g)+O_2(g) is k_I = 3.38 times 10^-5 s^-1 at 25 degree C. What is the half-life of N205? What will be the pressure, initially 500 Torr, after 50 20 min after initiation of the reaction?
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?
Using the following reactions: N_2(g) + O_2(g) rightarrow 2 NO(g) Delta H = 181 kJ times 2 NO(g) + O_2 rightarrow 2 NO_2(g) Delta H = -113 kJ times 2 N_2O(g) rightarrow 2 N_2(g) + O_2(g) Delta H = -163 kJ times Determine the enthalpy change for the reaction: N_2O(g) + NO_2(g) rightarrow 3 NO(g) Delta H =
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?...