For the reaction at 298 K,
2NO2 g → N2O4 g
the values of ΔHo and ΔSo are -58.0 kJ and -177 J/K, respectively. What is the value of ΔG nonstandard at 298 K when the concentration of N2O4 is 1.69 M and the concentration of NO2 is 2.75 M? Remember to answer in correct units.
ΔG=
For the reaction: 2NO2 (g) ↔ N2O4 (g) at 298 K, The value of ∆H⁰ and ∆S⁰ are -58.03 kJ and -176.6 J/K, respectively. (a) What is the value of ∆G⁰ at 298 K? (b) At what temperature would this process be spontaneous?
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298 K. N2O4(g)N2O4(g) NO2(g)NO2(g) S0S0 (J/K/mol) 304.29 240.06 ΔfH0ΔfH0 (kJ/mol) 9.16 33.18 Select one or more: A. Kp=9.23Kp=9.23 , Kc=12.3Kc=12.3 B. Kp=0.563Kp=0.563 , Kc=0.33Kc=0.33 C. Kp=0.144Kp=0.144 , Kc=0.0058Kc=0.0058 D. Kp=0.355Kp=0.355 , Kc=1.23
1. For the reaction at 298 K, P4O10s + 6H2O l → 4H3PO4s the values of ΔHo and ΔSo are -416 kJ and -209 J/K, respectively. What is the value of ΔGo at 298 K? Use correct units. ΔGo= 2. Will the following reactions show an increase or decrease for the value of ΔSrxn? NaCl s → Na+aq + Cl-aq H2O l → H2O g 2H2g + C s → CH4g 2CH3OH g + 3O2g → 2CO2g + 4H2O 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
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).
1. For the equilibrium reaction: 2NO2 - N2O4 a) calculate the literature values of ΔG°, ΔH° and ΔS° for the equilibrium reaction (ΔS° NO2 - 240.4 Jk/mol, N2O4- 304.3 Jk/mol) (ΔG° NO2- 51.839 KJ/mol, N2O4-98.286 KJ/mol) (ΔH° NO2 -33.85 KJ/mol, N2O4- 9.660 KJ/mol) b) From your understanding of the principals of FTIR spectroscopy, why is it that you do not see absorbance peaks for N2 gas but you do see them for NO2 and N2O4?
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔrH∘=55.3kJmol−1 At 298 K, a reaction vessel initially contains 0.100 bar of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 369 K? Assume that the initial pressure of N2O4 is the same (0.100 bar)
Consider the following reaction: 2NO2(g) ⟶ N2O4(g) Part B Calculate AG at 298 K if the partial pressures of NO2 and N204 are 0.39 atm and 1.62 atm , respectively. Express the free energy in kilojoules to two decimal places. PO AQ R o aj ? AG = Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
The value of Kc for the the following reaction is 0.470 at 471 K. N2O4(g)---->2NO2(g) Part 1) If a reaction vessel at that temperature initially contains 0.0200 M NO2 and 0.0200 M N2O4, what is the concentration of NO2 at equilibrium? _______M? part 2) What is the concentration of N2O4 at equilibrium? _______M?