Editing revision 4 of Review Homework For Equilibrium - Revised 2018
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<br> 1. For the following reversible reaction, <br> <Br> 3 H<sub>2 (g)</sub> + 1 N<sub>2 (g)</sub> <==> 2 NH<sub>3 (g) </sub> + Energy<br> <br> <br> a) Write the Equilibrium constant expression for this reversible reaction.<br> <br> <br> <br> <br> b) For the reversible reaction above, I found that I have the following equilibrium concentrations, what is Equilibrium constant ( K ) and its units.<br> [H<sub>2 (g)</sub>]<sub>E</sub> = 0.431M, [N<sub>2 (g)</sub>]<sub>E</sub> = 0.673M, and [NH<sub>3 (g)</sub>]<sub>E</sub> = 2.91M, <br> <br> <br> <br> <br> <br> c) Simply state next to each of the following stresses on the above equilibrium system, if the equilibrium will 1) shift to the Right, 2)shift to the Left, or 3) No shift in equilibrium<br> <br> i. Decrease Temperature<br> <br> <br> <br> <br> ii. Adding a compound that will consume N<sub>2 (g)</sub><br> <br> <br> <br> <br> d) If the above reversible reaction did not have the Equilibrium constant you calculated in Question 1b, but instead had a value of K = 1000. That would indicate that you have MORE PRODUCT or MORE REACTANT in your Equilibrium system. Circle the appropriate answer.<br> <br> <br> 2. Do you need the reactants to have the same concentration of reactants as the products to be at Equilibrium. Yes or No (Circle Correct answer). <br> <br> 3. Explain what Dynamic Equilibrium means.<br> <br> <br> <br> <br 4. Explain why the definition of Equilibrium and the Gibbs Free Energies differences are zero.<br> <br> <br> <br> <br> <Br>
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