Decomposition of nitrogen dioxide into nitrogen oxide gas is an equillibrium process described by the following equation: 2NO2(g)--2NO(g)+ O2(g), deltaH=-98.7kj. Predict whether the position of equilberium will shift to the right left or no change.
-increase the concentration of NO
-Decrease the concentration of NO2
-Increase the pressure by the addition of helium gas
-Increase the pressure by decreasing the volume
- Decrease the temp
-Add a catalyst
Decomposition of nitrogen dioxide into nitrogen oxide gas is an equillibrium process described by the following...
Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark-brown gas: 2NO(g) + O2(8) - 2NO2(8) In one experiment 1.075 mole of NO is mixed with 0.722 mole of O2. Calculate which of the two reactants is the limiting reagent, and report the number of moles of NO2 produced.
Answer is A 47. The oxidation of nitric oxide to nitrogen dioxide is 2NO(g) + O2(g) + 2NO2(g) If 100.0 mL of NO (at STP) reacts with 400.0 mL of O2 at STP, calculate the partial pressure of NO2 in the final reaction mixture. A) 0.222 atm B) 0.333 atm C) 0.286 atm 0.250 atm E) 1.00 atm
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...
Nitrogen dioxide gas undergoes decomposition producing nitrogen monoxide and oxygen gases: 2 NO2(g)........ 2 NO(g) + O2(g) A sample consisting of 0.10 moles of NO2 is placed in a 10.0 L in a container that is then heated to 750 K. When equilibrium is reached, the pressure in the container is 0.827 bar. Calculate the equilibrium constant and the degree of dissociation at this temperature. (Hint: pressures are directly proportional to concentration, so they can be used in ICE tables).
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 reversible decomposition of dinitrogen tetroxide, N, O, to nitrogen dioxide, NO,, is shown. For this reaction, Keq = 0.15. = NO dinitrogen tetroxide 2NO, nitrogen dioxide At equilibrium, is the concentration of reactants or products greater? The concentration of reactants equals the concentration of products at equilibrium. The concentration of products is greater than the concentration of reactants at equilibrium. The concentration of reactants is greater than the concentration of products at equilibrium Consider this system at equilibrium. PC12(g)...
II Review Constants Peri Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2(g) + 2NO(g) + O2(g) Part A In a particular experiment at 300°C, NO2 drops from 0.0100 to 0.00750 M in 100 s. The rate of appearance of O2 for this period is M/s. X 2.5 x 10-3 OOOOO 5.0 x 10-3 5.0 x 10-5 2.5 x 10-5 1.3 x 10-5 Submit Request Answer
Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2→2NO+O2 In a particular experiment at 300 ∘C, [NO2] drops from 0.0256 to 0.00889 M in 383 s . The rate of disappearance of NO2 for this period is ________ M/s. 1) 4.36×10−5 2) −9.01×10−5 3) 8.73×10−5 4) 2.29×104 5) 2.18×10−5
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?
Nitrogen dioxide, NO2 decomposes into nitrogen monoxide (NO) and oxygen gas O2, according to the following reaction. 2 NO2(g) → 2NO(g) + O2(g) A sample of nitrogen dioxide in a sealed vessel, and the total pressure in the vessel was measured to be 0.0980 atm before any reaction had occurred. The total pressure in the vessel was monitored over time during the reaction at 575 K, giving the following data. (a) (20 points) Determine the rate law (in pressure) for this reaction at 575...