calculate ΔGrxn at 36 ∘C. N2O4(g)→2NO2(g)
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Calculate ΔGrxn for the dissociation of N2O4 at 25°C with P(N2O4) = 0.150 bar and P(NO2) = 0.100 bar. Use the data provided below. ΔG°f (kJ/mol) N2O4(g) 99.8 NO2(g) 51.3
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
N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) c) Based on the K value calculated in 4c, which of the following is true about the reaction when it is performed at 100˚C? Select one or more: a. The reaction is nonspontaneous. b. The reaction is spontaneous.
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.
Given the reaction below: N2O4(g)→2NO2(g)N2O4(g)→2NO2(g) d) You increase [NO2][NO2], but change nothing else about the system. How will this affect the value of K? Select one: a. K will decrease. b. K will increase. c. K will not change.
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
Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant if the reaction is reversed: 2NO2(g) ↔ N2O4(g) ? A. -0.211 B. 0.211 C. 4.74 D. -4.74
Consider the following reaction: N2O4(g)⇌2NO2(g),Kc=0.36 at 2000∘C The reaction mixture initially contains only the reactant, [N2O4]=0.0300M , and no NO2. Find the equilibrium concentration of N2O4. Find the equilibrium concentration of NO2.
Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant is the reaction is balanced as ½ N2O4(g) ↔ NO2(g) ? A. 0.106 B. 0.459 C. 0.211 D. 0.422
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! Thank you for your help!