Question

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MUUUUUUIU. PIBB show all WOPR Poquim Gulauons, By t proper units, etc. Work alone and return this written copy in with your answers at the beginning of the following lecture meeting. "NOTE: Total of 60 out of 55 points possible! This 5 points of extra credit possible, in addition to the extra credit applied to your final grade. 1. Match the following (12 points) Answer Concept A OH Description 1. Applying heat retards the formation of product 2. Conjugate acid of water B. Shift toward reactants C. Shift toward products D. H30' 3. Conjugate base of water 4. Applying heat promotes the formation of product 5. Solute resulting in a neutral solution 6. KEQ 7. K.> QC 8. KQ E. NHACH3COO F. Equilibrium G. Exothermic reaction H. Endothermic reaction 2. A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L system. The following equilibrium is established at 500 K CO2(g) + H2g) -> CO + H2O) At equilibrium, Pro - 3.51 atm. A) Calculate the equilibrium partial pressures of CO2, Hz, and CO (6 points) and B) Calculate ko for the reaction (4 points). Recall PV = nRT, with R = 0.0821 L-atm/mol-K. Hint: ICE chart not necessary. Notice how CO and H2O are equivalent, stoichiometrically.

Answer 1

1.

1. Exothermic reaction: In an exothermic reaction heat is generated along with the formation of products so if we apply heat the product formation is retarded in accordance with Le Chatelier Principle. ( Le Chatelier Principle states that if a system in chemical equilibrium is subjected to a disturbance it tends to change in a way that opposes this disturbance.)

2. H₃O⁺ . As a rule of thumb, the conjugate acid is simply the original species with an additional proton, H+ whereas the conjugate base is the original species MINUS a proton, H⁺ .

3. OH^-is the conjugate base of water.

4. Endothermic reaction: In these reactions product formation is accompanied by absorption of heat from the surroundings. So in accordance with Le Chatelier Principle applying heat will promote product formation by shifting the equilibrium in the direction of products.

5. NH₄CH₃COO: When this salt is hydrolyzed it forms NH₄⁺ and CH₃COO ^- . The k_b value of NH₄⁺ is equal to the k_a value of CH₃COO ^- . Due to which they neutralize each other and the resultant solution is neutral.

6. Equilibrium.

Q_C = Reaction quotient and K_C = equilibrium constant. At Q_C = K_C the system is at equilibrium.

7. Shift towards products.

When K_C > Q_C , there are more reactants than products. Some of the reactants will become products, causing the reaction to shift towards the products.

8. Shift towards reactant.

When K_C < Q_C , there are more products than reactants. To decrease the quantity of products, the reaction will shift to the left and produce more reactants.

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