### Chemical Equilibrium and Reaction Yield **Question:** Which change would increase the production of water vapor (H₂O) in this reaction? \[ 2H_2S(g) + 3O_2(g) \leftrightarrow 2H_2O(g) + 2SO_2(g) \] **Options:** - O Adding SO₂ - O Removing H₂S - O Decreasing pressure - O Removing SO₂ **Answer Explanation:** In this chemical reaction, the formation of water vapor (H₂O) as a product is considered. To increase the production of water vapor, we need to shift the equilibrium position of the reaction towards the products side (right side of the reaction equation). By Le Chatelier’s principle, changes in concentration, pressure, and temperature can shift the equilibrium position in a predictable way: **Options Analysis:** 1. **Adding SO₂:** This would increase the concentration of a product, thereby shifting the equilibrium to the left, decreasing the production of H₂O. 2. **Removing H₂S:** This would decrease the concentration of a reactant, shifting the equilibrium to the left, and thus decreasing the production of H₂O. 3. **Decreasing Pressure:** The reaction has equal volumes of gaseous reactants (5 volumes) and gaseous products (4 volumes). Decreasing pressure favors the side of the reaction with more gas molecules, which is the reactants side in this case. Hence, it would decrease the production of H₂O. 4. **Removing SO₂:** This would decrease the concentration of a product, shifting the equilibrium to the right to produce more H₂O and SO₂. **Correct Option:** - **Removing SO₂** Removing one of the products will shift the equilibrium to the right, thus increasing the production of water vapor (H₂O). Students should consider the concepts of chemical equilibrium and Le Chatelier's principle when solving similar problems.

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-

For the reaction H2(g) + Br2(g) =2 HBr(g), Kc = 81.4 at 385°C. If [H2] = [Br2] = [HBr] = 2.4 x 10-4 M at 385°C, which one of the following is correct? %3D [HBr] increases as the system approaches equilibrium. [H2] and [HBr] decreases as the system moves toward equilibrium. [H2] and [Br2] increases as the system approaches equilibrium. There is not enough information given to make a determination. [HBr] and [Br2] increases as the system approaches equilibrium. The system is at equilibrium.

The equilibrium reaction of 2 moles of SO2e) plus 1 mole of O2e) produces 1 mole of SO3@)- What is the equilibrium constant expression for this reaction. 2(g)

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NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.

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For the reaction N2 (g) 02 (g) = 2 NO (g) Kc = 1.00 x 10P at 1200 °C. if 0.675 mol N2 and 0.675 mol O2 are placed in a 10.00 L container maintained at 1200 °C, what will be the concentration of NO (g) at equilibriu O 1.064 x 10 3 M O 2.128 x 10 3 M O 1.481 x 10-4 M 2.128 x 10-4 M O 1.064 x 10-4M A Moving to another question will save this response.

24. The following reaction takes place: A,B = 2A + B + heat. If 4.00 moles of A,B is added into a 1.00 L container, it is found that 32.0 % of the reactant dissociates to reach equilibrium. Create an ICE table and solve for the Keg of this reaction. Note: Show all calculations, follow the rules of significant figures, and box your final answer.