Given the same reactant concentrations, the reaction CO(g) + Cl_2(g) rightarrow COCl_2(g) at 263 degree C...
13.38 Given the same reactant concentrations, the reaction CO(g) + Cl2(g) — COC12(8) at 250°C is 1.50 x 10 times as fast as the same reac- tion at 150°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
Enter your answer in the provided box. Given the same reactant concentrations, the reaction CO(g) + Cl2(g) COCl2() at 235°C is 54.3 times as fast as the same reaction at 157°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant. kJ/mol
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) + NO_3(g) (Slow, endothermic) NO_3(g) + CO(g) rightarrow NO_2(g) + CO_2(g) (Fast, exothermic) a) Write the overall reaction. b) Identify each of the following as a reactant, product, , or intermediate, NO_2, CO, NO_3, CO_2, NO. c) Draw a reaction coordinate for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change. d) Give a plausible rate law.
For the reaction 2 HBr(g) + Cl_2(g) rightarrow 2 HCl(g) + Br_2(g) a. Write the equilibrium constant expression for the reaction. b. Using the following G degree values, calculate Delta G degree for the reaction. HBr(g) = -53.22 kJ/mol HCl(g) = -95.27 kJ/mol Cl_2(g) = 0 kJ/mol Br_2(g) = 3.14 kJ/mol c. Calculate the equilibrium constant K_eq be at 298 K. d. Does this equilibrium lie more with reactants or products?
Consider the following reaction where K_c = 77.5 at 600 K. CO(g) + Cl_2(g) COCl_2(g) A reaction mixture was found to contain 2.42 times 10^-2 moles of CO(g), 4.19 times 10^-2 moles of Cl_2(g) and 0.121 moles of COCl_2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q_c, equals The reaction must run in the forward direction to reach equilibrium. must run in...
What is Delta G in kJ for the reaction: Cl_2(g)+ 2 Br^- rightarrow Br_2(l) + 2 Cl^- if [Br^-] = 0.100, [Cl^-] = 0.50, and p(Cl_2) = 1.00 atm? The temperature 25 degree C.
Consider the reaction: l_2(g) + Cl_2 (g) 2lCl(g); K_p = 81.9 at 25 degree C. Calculate the standard free energy change for this reaction.
For the following reaction at 25.0 degree C, 2 C(s) + O_2(g) rightarrow 2 CO(g) calculate Delta S degree_univ given Delta S degree_sys = 179.1 J/K and Delta H degree_sys = -221.1 kJ.
The reaction NO(g) + 7/2 Cl_2(g) rightarrow NOCl(g) is first-order in [Cl2] and second order with respect to [NO]. Under a given set of conditions, the initial rate of this reaction is 6.20 times 10^-6 mol/L s. What is the rate of this reaction if the concentration of NO is doubled and the concentration of Cl_2 is reduced to half the original value? 6.20 times 10^-6 mol/L s 2.48 X 10_5 mol/L s 1.24 times 10^-5 mol/L s 4.96 times...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal to 512 M^-1 S^-1. If the initial concentration of Mn(CO)_5 is 0.011 M, how long will it take for the reactant concentration to reach 0.0011 M? Units: s a. 1.6 b. 5.1 c. 0.020 d. 0.28 A plot of a 1/[A] versus time gave a straight line. This indicates that A rightarrow B + C a. the reaction is zero order in reagent A...