The reaction N2O4(g) ⇌ 2NO2(g) has ∆G° = 13.3 kJ/mol at 25 °C. What is the...
The reaction N2O4(g) ⇌ 2NO2(g) has ∆G° = 13.3 kJ/mol at 25 °C. What is the value of ∆G, in kJ/mol, for this reaction at this temperature when [N2O4] = 3.0 M and [NO2] = 0.0010 M? Enter your answer to the tenths place. Do not include units. Include the sign if appropriate!
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The reaction N2O4(g) ⇌ 2NO2(g) has ∆G° = 13.3 kJ/mol at 25 °C.
What is the...
For the reaction at 298 K, 2NO2 g → N2O4 g the values of ΔHo and...
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=
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298...
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
For the following reaction : 2NO2(g) ? N2O4(g) ?H� = -58.04 kJ/mol Try to predict what...
For the following reaction : 2NO2(g) ? N2O4(g) ?H� = -58.04 kJ/mol Try to predict what happens to the system at equilibrium if: a/ The temperature is raised? b/ The pressure of the system is increased? c/ An inert gas is added to the system at constant pressure? d/ An inert gas is added to the system at constant volume? e/ A catalyst is added to the system?
1. For the equilibrium reaction: 2NO2 - N2O4 a) calculate the literature values of ΔG°, ΔH°...
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?
The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2]...
The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2] = 0.047 M , what is the molar concentration of N2O4? Express the concentration to two significant figures and include the appropriate units.
For the reaction N2O4(g)⇌2NO2(g), the value of K at 25∘C is 7.19×10−3. Calculate [NO2] at equilibrium...
For the reaction N2O4(g)⇌2NO2(g), the value of K at 25∘C is 7.19×10−3. Calculate [NO2] at equilibrium when [N2O4]=6.90×10−2mol/L.
Decomposition of nitrogen dioxide dimer N2O4 is described by the reaction: N2O4(g) = 2NO2(g) Concentration of...
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
Calculate the equilibrium concentrations of N2O4and NO2 at 25 ∘C if the initial concentrations are [N2O4]=...
Calculate the equilibrium concentrations of N2O4and NO2 at 25 ∘C if the initial concentrations are [N2O4]= 0.0150 M and [NO2]= 0.0360 M. The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. Part A Calculate the equilibrium concentration of N2O4. Express your answer with the appropriate units. Part B Calculate the equilibrium concentration of NO2. Express your answer with the appropriate units.
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf...
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
The value of Kc for the the following reaction is 0.470 at 471 K. N2O4(g)---->2NO2(g) Part 1)...
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?
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