The Kc for the reaction at 298 K is given
N2O4(g) ⇋ 2 NO2(g) Kc = 5.9 × 10–3
What is the Kc for the following reaction?
½ N2O4(g) ⇋ NO2(g) Kc = ?
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc =...
Find ΔrG for reaction (in kJ mol-1) at 298 K? 2 NO2 (g) ⇌ N2O4 (g) Given Conditions: Pressure: NO2 = 1.25 bar Pressure: N2O4 = 0.65 bar N2O4(g) --
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 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=
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?
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
1) Kc = 45 for the equilibrium : 2 NO2(g) <====> N2O4 (g) at a temperature 85 C a) What is Kc for N2O42 <====> NO2(g) ? b) What is Kp for 2 NO2(g) <====> N2O4 (g) at 85 C? R= 0.0821 L-atm/ k-mol 2) The pH of seawater is 8.10 This corresponds to ________ M H+
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...
Calculate Kp for the following (R = 0.08206 L.atm/mol.K): a) N2O4(g) ->2NO2(g) Kc = 5.9 x 10 -3 (at 298 K) b) N2(g) + O2(g) -> 2NO(g) Kc = 4.10 x 10 -31 (at 298 K)
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
The value of Kc for the the following reaction is 0.470 at 473 K. N2O4 = 2NO2 If a reaction vessel at that temperature initially contains 0.0250 M NO2 and 0.0250 M N2O4, what is the concentration of NO2 at equilibrium? What is the concentration of N2O4 at equilibrium?