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2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related...
3. Given Kc or Kp for the following reactions, what is the value of Kp or Ke? (a) 12 (g) + Cl2 (a) 22ICI (g): Kc = 2.0 x105 at 25°C (b) N204(g) + 2NO2(0); Kc = 0.90 at 120 °C (c) CaCO3(s) = Cao (s) + CO2 (ox Kp = 1.67 x 102 at 740 °C 4. A container contains an equilibrium mixture of H2 (g), 12(g), and Hl) at 721 K. The concentration of each substance present at...
. Determine the value of the equilibrium constant for the reaction N2 (g) + 2O2 (g) ↔ N2O4 (g) from the following equations. ½ N2 (g) + ½ O2 (g) ↔ NO (g) KC = 6.9 x 10-16 2NO2 (g) ↔ 2NO (g) + O2 (g) KC = 4.5 x 10-13 2NO2 (g) ↔ N2O4 (g) KC = 6.7
Can you work this question with the work all step by step? 3. Given Kc or Kp for the following reactions, what is the value of Kp or Ke? (a) 12 ) + Cle) = 2ICI) Ke = 2.0 x105 at 25°C (b) N2040 = 2NO2) : Ke = 0.90 at 120°C (c) CaCO3) = Cao (s) + CO2(g): Kp = 1.67 x 102 at 740 °C
3. Given Koor Kp for the following reactions, what is the value of Koor K? (a) 12 (g) + Cl2 (g) = 2ICI (9) Kc = 2.0 x105 at 25°C (b) N204 () = 2NO2(g) ; K = 0.90 at 120 °C (c) CaCO3 (s) : CaO (s) + CO2 (g) Kp = 1.67 x 102 at 740 °C
True or False t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...
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 below the Kc is 56.4, determine the concentration of O2 at equilibrium if the concentration of N2 is 0.0013 M and the concentration of NO2 is 0.00065 M. N2 (g) + 2O2 (g) ⇌ 2NO2 (g) 0.0089 M 0.0024 M 0.042 M 0.016 M
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.26, 0.36, and 0.030 atm, respectively, at 2200°C, what is KP?
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.20, 0.35, and 0.030 atm, respectively, at 2200° C, what is KP?
2. Determine Ke for the reaction (Answer: 9.7x10-16): 2 N2(g) + 1/2O2(g) + Brz(g) $ NOBr (g) From the following information (Hint: Manipulate the equations first, then manipulate K values): 2 NO(g) 5 N2(g) + O2(g) NO (g) + Br2 (g) $ NOBr (g) Ke=2.1x1030 Ko=1.4