7. Calculate the rate constant at 70°C for the reaction A + 3B-> 2C given that...
Calculate the activation energy of a reaction if the rate constant at 555 K is 3.72 times 10^-5 and at 761 K it is 2.95 times 10^-3. Calculate the rate constant at 70 degree C for the reaction A + 3B rightarrow 2C given that the rate constant of the reaction is equal to 3.5 times 10^-1 M^-4 s^-1 at 95 degree C. (Ea = 142 kJ/mol)
7. If AGfor the reaction A(aq) + 3B(aq) - 2C(aq) + D(aq) is equal to-43.85 kJ, what is AG at 350 K IF(A=0.12 M. [B]=0.38 M, and [C]=[D]=0.54 M? 8. Given the reaction CS2(9)+CS (), calculate AS gur if AH -27.7 kJ and T-300K. 10. Balance the following redox reaction in acidic solution: MnO4 (aq) + CHaq) -- Mn"(aq) + Cl(a).
Consider the generic reaction: 2A + 3B --> 2C Hrxn = -100 kJ If a reaction mixture initially contains 5 mol of A and 6 mol of B, how much heat (in kJ) will have evolved once the reaction has occurred to the greatest extent possible?
39. Given the following reaction: 2C2Hs + 70, > 4CO2 + 6H20 And given: 2H2 + O2 → 2H20 C+02 0 2C + 3H2 → GH AH = 384. kl/mol AH = -394. kl/mol AH = 192.0 kJ/mol Calculate the energy produced if 20. grams of CHe burn in air? 40) Write abbreviated condensed) configurations (noble gas core) for the following a. Chromium b. N.
If a temperature increase from 10.0 ∘C to 22.0 ∘C doubles the rate constant for a reaction, what is the value of the activation barrier for the reaction? Ea = nothing kJ/mol Exercise 14.71 < 28 of 32 (> A Review | Constants Periodic Table Part A If a temperature increase from 10.0°C to 22.0°C doubles the rate constant for a reaction, what is the value of the activation barrier for the reaction? Yo AL O O ? Eq =...
If the rate constant for a particular reaction triples between 35 °C and 70 °C, calculate the value of the activation energy for the reaction. A.1.92 kJ B.272 kJ C.82.7 kJ D.27.6 kJ E.0.639 kJ
Given A + 3B 2C + D This reaction is first order with respect to reactant A and second order with respect to reactant B. If the concentration of A is doubled and the concentration of B is halved, the rate of the reaction would ________ by a factor of _______.
Calculate the rate constant at 200.°C for a reaction that has a rate constant of 4.10 × 10−4 s−1 at 90.°C and an activation energy of 57.3 kJ/mol.
Calculate the rate constant at 225 degrees C for a reaction that has a rate constant of 8.1 x 10^-4 s^-1 at 95 degrees C and an activation energy of 95.0 kj/mol
2. Calculate the equilibrium constant of the overall reaction: 2A + 3B 4C given that these equations are known: Keq = ? Rxn 1 Rxn 2 2A + 2B → C+D 3C+DB Kegl = 20 Keq2 = 5 a. 4 b. 15 c. 25 d. 100 e. 320 3. Write the equilibrium expression for the reaction