The rate constant for a first-order reaction is 1.8 times 10^-2 s^-1 at 690 K an

Question

The rate constant for a first-order reaction is 1.8 times 10^-2 s^-1 at 690 K and 3.6 times 10^-2 s^-1 at 876 K. What is the activation energy? 8.1 kJ/mol 19 kJ/mol 2300 kJ/mol 18 kJ/mol 8 kJ/mol Which of the following statements is true in a reaction system at equilibrium? The number of collisions per unit time between reactants is equal to the number of collisions per unit time between products. Reactants are reacting to form products at the same rate as products are reacting to form reactants. The product of the concentrations of the reactants divided by the product of the concentrations of the products is always a constant. Reactants and products are present in equimolar amounts For the reaction given below, 2.00 mol of A and 3.00 mol of D are placed in a 6.00-L container A (g) + 2B (g) C (g) At equilibrium, the concentration of A is 0.200 mol/L. What is the concentration of B at equilibrium? 0.200 mol/L 0.233 mol/L 0.500 mol/L 0.400 mol/L

Explanation / Answer

3) ln (K2/K1) = (Ea /R) (1/T1 - 1/T2)

T1 = 690 K K1 = 1.8 x 10-2 s-1

T2 = 876 K K2 = 3.6 x 10-2 s-1

ln (3.6 x 10-2  / 1.8 x 10-2) = (Ea / 8.314) (1/690 - 1/876)

0.693 = Ea / 8.314 (0.00145 - 0.00114)

0.693 / 0.00031 = (Ea / 8.314)

22354.84 = Ea / 8.314

Ea = 185858.14 J/mol

Ea = 185.8 KJ/mol

4) answer = option B

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