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Dinate for a reversible catalyzed and uncatalyzed reaction. Referring to the diagram, answer the questions that follow. 1. The reaction shown above is (a) endothermic, (b) exothermic. 10. Which lettered arrow represents activation energy for the forward catalyzed reaction? 2. Which lettered arrow represents the energy of the reactants for the forward reaction? 11. Which lettered arrow represents activation energy for the forward uncatalyzed reaction?.

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  1. Press the ‘Get Form’ button to access the Chemistry Form Ws7 5 2a and open it in your chosen editor.
  2. Begin by entering your name in the designated field at the top of the form.
  3. Fill in the date in the specified area after your name.
  4. Identify your class period and input that information where indicated.
  5. Proceed to the section titled 'Interpreting Reaction Coordinates'. Carefully examine the corresponding diagram provided.
  6. For each question numbered from 1 to 18, evaluate the diagram and select the correct answer, marking it as (a) or (b) where necessary according to the instructions.
  7. Ensure all answers are based on your understanding of the reaction coordinate and the concepts of kinetics and equilibrium.
  8. Review your entries for any errors or omissions before finalizing.
  9. Once you have completed the form, you can save your changes, download a copy, print it, or share it as needed.

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Adding more reactants shifts the equilibrium in the direction of the products; therefore, the equilibrium shifts to the right.

Catalyst does not affect the position of equilibrium and hence it does not have any effect on the value of equilibrium constant.

Changing temperature Increasing the temperature decreases the value of the equilibrium constant. Where the forward reaction is endothermic, increasing the temperature increases the value of the equilibrium constant. The position of equilibrium also changes if you change the temperature.

Increasing the system volume shifts the equilibrium to the right. 27. At 250ºC, the equilibrium constant Kp for the reaction PCl5(g) ↔ PCl3(g) + Cl2(g) is 1.80.

Equilibrium shifts to the right. That is, when a new equilibrium is reached (when the rate of forward and reverse reactions are equal again), there will be more product than before. When the concentration of reactants is increased, the equilibrium shifts to the right and there will be more product than before.

The temperature dependence of the equilibrium constant is generally determined by of the reaction. As the temperature increases, the equilibrium constant for an exothermic reaction ( ) decreases. For the endothermic reaction ( ), the equilibrium constant increases as the temperature increases.

Increasing the concentration of a reactant causes the equilibrium to shift to the right, producing more products. Increasing the concentration of a product causes the equilibrium to shift to the left, producing more reactants.

Changing the concentration If one of the products is removed from a reaction (on the right), then the position of equilibrium moves to the right to make more of that product.

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