For the dimerization of nitrogen dioxide, ΔG° = −4.7 kJ at 25°C. 2 NO2(g) ⟶ N2O4(g) Calculate ΔG for this reaction if the partial pressures of NO2 and N2O4 are both 0.38 atm. (R = 8.31 × 10−3 kJ/K)
a. -10.86 kJ
b. -11.36 kJ
c. -15.12 kJ
d. -11.07 kJ
e. -7.10 kJ
For the dimerization of nitrogen dioxide, ΔG° = −4.7 kJ at 25°C. 2 NO2(g) ⟶ N2O4(g)...
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Consider the reaction 2 NO2(g) →N2O4(g) .(a) Using ΔGfN2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K.kJ(b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.25 atm and 1.30 atm, respectively.kJ
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...
A flask is charged with 1.500 atm of N2O4(g) and 0.94 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below. N2O4(g) 2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. (a) What is the equilibrium partial pressure of N2O4? ______ atm (b) Calculate the value of Kp for the reaction. ______ (c) Is there sufficient information to calculate Kcfor the reaction? -Yes, because the temperature is specified. -No, because the value of...
Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k = 2.5 × 103 s–1 at –5°C and k = 4.7 × 103 s–1 at 25°C, what is the activation energy for the decomposition? Select one: A. > 1000 kJ/mol B. 580 kJ/mol C. 0.73 kJ/mol D. 58 kJ/mol E. 14 kJ/mol
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
Dinitrogen tetroxide decomposes to nitrogen dioxide. Write the balanced chemical equation for this reaction. Start with pure N2O4 at 1.00 atm. Find the equilibrium partial pressures of N2O4 and NO2. The equilibrium constant for this reaction is K = 11.
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...
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn= 55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 380 K ? Assume that the initial pressure of N2O4 is the same (0.100 atm).
A flask is charged with 1.800 atm of N2O4(g) and 1.00 atm of NO2(g) at 25 ∘C , and the following equilibrium is achieved: N2O4(g)⇌2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.519 atm . 1A) What is the partial pressure of N2O4 at equilibrium? 1B) Calculate the value of Kp for the reaction. 1C) Calculate the value of Kc for the reaction.