Each step represents an elementary reaction. Step1.       A + 2B  ↔  C         (fast equilibrium, k1 and k-1) Step2.       C + D   →  E          (slow, k2)   a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the

Reaction 1 Reaction Progress 6. A(g) + B (g) →C(g) For the reaction above AH=+100 KJ. The forward reaction starts slowly but speeds up when a catalyst is added. Below write out a potential energy diagram for the reaction. Be sure to label the following on your diagram: a. Both axes b. Product and reactant energy c. Activated complex energy d. Sketch the curve e. Activation energy f. Enthalpy

Consider the following reactions: + O2(e) + O2(8) + 2H* → 2NO(8) → 2MgO(s) I. II. N2e) Mg(s) (aq) > Ca2+ Increasing the surface area will increase the reaction rate in: II. CaCO3(s) + H2Ou + CO2(8) (aq) А. Il only В. I and III only C. Il and III only D. I, II, and III

Which one of the following factors does not affect the specific rate constant of a chemical reaction?   A.  Arrhenius probability factor   B.  Temperature   C.  Activation barrier   D.  The presence of a catalyst   E.  Change in the Gibbs free energy for the reaction

9. An increase in temperature increases the reaction rate. What is the best reason to explain this effect? A. a greater fraction of the collisions have the correct orientation of molecules B. the activation energy of the reaction will increase C. the activation energy of the reaction will decrease D. more collisions will have enough energy to exceed the activation energy

just need help with d and e please

What is the value of one mole?

7. Reactions A and B were studied and found to produce the given energy diagrams. 150 150 Energy 100 (kJ/mol) 100 Energy (kJ/mol) 50 50 Reaction progress Reaction progress Reaction A Reaction B A third reaction, C was studied with a measured activation energy of 55 KJ/mol. Assume all reactions take place at the same temperature. Reaction A is slowest a. b. Reaction B is slowest c. Reaction C is slowest d. All reactions happen at the same rate.

Chemistry

a. Will the reaction happen? Explain your answer in detail with how the bonds will form. b. Explain in detail 2 ways that the molecules can be affected to speed up the rate of the reaction. 70 kJ Reactants N Activation Energy FF 50 kJ Products FN F 10 kJ Reaction Progress E'E N 10 kJ Potential Energy [kJ]