Name NO2 Nitrogen dioxide Nitrite O hyponitrite O nitrogen(IV) oxide O none of these
itric oxide (NO) and oxygen (O2) react in the atmosphere to form nitrogen dioxide (NO2), an air ollutant that causes lung irritation. - Write the balanced chemical equation for this reaction. Complete the reactant side of this representation for the reaction of NO and O2 to form NO2. •=0 O=N Before Reaction After Reaction
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...
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.
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
Question 16 5 pts Nitrogen dioxide dissociates to form nitric oxide and oxygen 2 NO2)2 NO(g) + O2(8) What is value of the equilibrium constant for the reverse reaction if the equilibrium concentration of NO2 is 0.240 M, NO is 0.112 M, and O2 is 0.360 M at 33°C? 0108 0.0784
Measurement of nitrogen in water in the form of nitrite NO2- can be achieved by diazo dye formation followed by measurement of absorbance at 543 nm. Measurement of nitrate nitrogen (NO3-)is achieved by reducing the nitrate to nitrite then determining total nitrite nitrogen, nitrate nitrogen is found by difference. The following calibration data were used in nitrate-and nitrite nitrogen determinations: mg nitrogen. L-1 as nitrite absorbance at 543nm 0.000 0.000 0.050 0.055 0.100 0.111 0.200 0.218 0.500 0.556 A undiluted...
carbon monoxide reacts with nitrogen dioxide to produce carbon dioxide and nitric oxide as given by the following reaction. CO (g) + NO2 (g) → CO2 (g) + NO (g) The reaction is zeroth order in CO and second order in NO2, and second order overall. The rate constant for this reaction at 175ºC is 7.58 × 10-4 L mol-1 s-1. If the initial concentration of NO2 was 0.565 M, what is the molar concentration of NO2 after 5.8 minutes?...
Calculate ΔH° for the oxidation of nitric oxide to nitrogen dioxide, 2 NO(g) + O2(g) ---> 2 NO2(g), from the following data: ΔH°f[NO(g)] = +90.25 kJ/mol ΔH°f[NO2(g)] = +33.18 kJ/mol +16.93 kJ/mol -218.71 kJ/mol -114.14 kJ/mol -172.15 kJ/mol +69.54 kJ/mol
Nitrogen dioxide reacts with carbon monoxide to produce nitric oxide as follows: NO2 (9) + CO (9) ► NO (9) + CO2 (g) The reaction is second order in NO2, zeroth order in CO and second order overall. How long (in hours) will it take for NO2 to decompose by 35.8% given the initial concentration was 0.43 M NO2 and CO was in excess. The rate constant for this reaction at 225°C is 2.08 x 10-4 L/mol/s. Report your answer...
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