Sketch a graph for each situation The reactants have a lower potential energy than the products. The activation energy of the reverse reaction is greater than the forward reaction. The products have a lower potential energy than the reactants. The forward reaction has a positive DH. The reverse reaction has a negative DH. Thank you!

The following figure represents chemical reaction before and after using a catalyst and from the figure it is obvious that 300 a-catalyst preserve heat energy its value is 100KJ/mol on the usage of the catalyst 100 Reactant b-this reaction is endothermic Product -100- c-activation energy of the forward reaction with out a catalyst is 200KJ/mol d-the catalyst increases energy of reactants which increases rate of the reaction Progress of reaction Energy,(k/mol)

Consider a hypothetical chemical reaction: A+B C+D (In this equation A, B, C and D stand for some unknown chemical formulas.) Here is an energy diagram for the reaction: energy (kJ/mol) 400 Explanation 300- 200 100 0 A + B C + D reaction coordinate Use the energy diagram to answer these questions. Check Muumal

Which one of the following statement is true about how catalyst works? Catalysts increase the rate of reaction by decreasing activation energy. Catalysts are used up in the reaction to increase the rate. Catalysts decreases the rate of reaction by speeding up the reverse reaction. Catalysts increases the rate of reaction by releasing heat.

Q20

Question 8 In an endothermic reaction, the collision energy of the reactants will be greater than that of the products. the forward reaction is slower than the reverse reaction. O the reaction rate will speed up with time. the forward reaction will have a greater activation energy than the reverse reaction. O the activation energy will change as the reaction progresses. Question 9

Typical Chemical Potential Energy (PE) Diagram for an Exothermic Reaction A catalyst provides an alternate pathway for a reaction to occur. The alternate pathway has a lower activation energy (AE), meaning that the reactant molecules do not need to collide with as much energy in order for a reaction to occur, so more collisions result in a reaction, so the reaction rate is faster. Chemical Potential Energy (Enthalpy) Note that adding a catalyst does not change the amount of energy released (AH) for the reaction. Activation Energy (AE) with a catalyst PE of Reactants AH PE of Products Rxn Progress What effect does a catalyst have on the stoichiometry of the reaction? What effect does the catalyst have on the mechanism of a reaction? AE wlo a catalyst

How does increasing temperature affect the rate of reaction?       the activation energy increases so the reaction rate decreases       the reactants have more kinetic energy so the frequency of the effective collisions increases       the reactants have more kinetic energy so the frequency of the effective collisions decreases       the activation energy increases so the reaction rate increases

The diagram shows the potential energy changes for a reaction pathway. B Reaction Pathway Part 1: Does the diagram illustrate an endothermic or an exothermic reaction? Give reasons in support of your answer. Part 2: Describe how you can determine the total change in enthalpy and activation energy from the diagram and if each is positive or negative. Potential Energy A

Referring to the reaction below, which of the following statements correctly describes the reaction to the given stress according to Le Chatelier's Principle? NH4HS(s)  ↔  NH3(g)  +  H2S(g)     Adding NH4HS will cause a shift toward products.     Adding NH3 will cause a shift toward products     Increasing the volume will cause a shift toward products.     Removing H2S will cause a shift toward reactants.