Question

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c. 5000 sec d. 31.25 min e. 27.1 min The rate constant for a certain chemical reaction is 0.00250 L mol's at 25.0 °C and 0.0125 mol's" at 50.0 °C. What is the activation energy for the reaction, expressed in ku? 1. a. 25.1 kJ b. 51.6 kJ C. 37.6 kJ d. 45.3 kJ e. 60.3 kJ 8. Using this data, 2 NO(g) + Cl2(g) = 2 NOCI(g) Kc = 3.20 x 103 2 NO2(g) = 2 NO(g) + O2(g) Kc = 15.5 calculate a value for Kc for the reaction, NOCI(9) + / 02(g) = NO2(g) + ) Cl2(g) a. 2.06 x 104 b. 4.84 x 10 c. 0.223 d. 4.49 e. 20.2 n o - 2 Soala at 900.0 Kthe equilibrium constant, Kc,

Answer 1

Answer & According to Arrhenius equation - en (K) - { [ 1 / 2 / Here K₂ and k are rate constants of a reaction at I and T, temperature (in kelvin) respectin Ea is activation energy Ris gas constant K₂ = 0.0125 L.motl.51 T2 = (273 +50k - 323k K = 0.00250 L-mot! 51 T = (273 +25) K = 298k R = 8.314 I/molok Ea - X 298 323 0.00250 0.0125 8.314 ar Ea=51518. Ea - 51518 J/mol - 51.5 kJ/mol option (6) is closest to obtained Hence option (6) is correct Ea value.