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.
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The reversible gas-phase decomposition of nitrogen tetra oxide,
N2O4, to nitrogen dioxide, NO2, is
to be...
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15. Consider the reaction 2 NO2(g) N2O4(g) . (a) Using Gf N2O4(g) = 97.79 kJ/mol and...
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N2O4(g) .
(a) Using Gf
N2O4(g) = 97.79 kJ/mol and Gf NO2(g)
= 51.3 kJ/mol, calculate G° at 298 K.
kJ
(b) Calculate G at 298 K if the partial pressures of
NO2 and N2O4 are 0.35 atm and 1.60
atm, respectively.
kJ
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The oxidation of nitric oxide NO + 02 =NO2 takes place in an isothermal batch reactor....
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Gaseous dinitrogen tetroxide(N2O4) decoposes to form nitrogen dioxide gas (NO2). Write a balanced equation for this...
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15. Consider the reaction 2 NO2(g)
N2O4(g) .
(a) Using Gf
N2O4(g) = 97.79 kJ/mol and Gf NO2(g)
= 51.3 kJ/mol, calculate G° at 298 K.
kJ
(b) Calculate G at 298 K if the partial pressures of
NO2 and N2O4 are 0.35 atm and 1.60
atm, respectively.
kJ
16. Consider the reaction given below.
H2(g) + F2(g)
2 HF(g)
(a) Using thermodynamic data from the course website, calculate
G° at 298 K.
kJ
(b) Calculate G at 298 K...
The oxidation of nitric oxide NO + 02 =NO2 takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 20.0 volume percent NO and the balance air at an initial pressure of 380 kPa (absolute). (a) Assuming ideal-gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of NO is 90%. (b) Suppose the pressure in the reactor eventually equilibrates (levels out) at 360 kPa. What...
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
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