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Suppose a 250. mL flask is filled with 1.2 mol of H₂ and 0.90 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I₂. You can leave out the M symbol for molarity. H₂ 1₂ HI П initial 1.2 0 ? change U equilibrium X 3

Suppose a 250. mL flask is filled with 1.2 mol of H₂ and 0.90 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I₂. You can leave out the M symbol for molarity. H₂ 1₂ HI П initial 1.2 0 ? change U equilibrium X 3

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Chemical Equilibrium Problem** **Scenario:** Suppose a 250. mL flask is filled with 1.2 mol of \(H_2\) and 0.90 mol of \(HI\). This reaction becomes possible: \[ H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \] **Instructions:** Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use \(x\) to stand for the unknown change in the molarity of \(I_2\). You can leave out the \(M\) symbol for molarity. **Table Descriptions:** | | \(H_2\) | \(I_2\) | \(HI\) | |----------|---------|---------|--------| | initial | 1.2 | | | | change | | \(x\) | | | equilibrium | | | | - **Initial Molarity Row:** This row lists the initial molarity of the reactants and products before the reaction starts. According to the given problem, the initial molarity of \(H_2\) is 1.2 M. - **Change in Molarity Row:** This row represents the change in concentration of each species as the reaction progresses towards equilibrium. The change in molarity of \(I_2\) is represented by \(x\). - **Equilibrium Molarity Row:** This row shows the concentrations of reactants and products once the equilibrium is achieved. These need to be calculated based on the initial conditions and the change in molarity \(x\). Remember, the values in the table are intended to be filled out with specific calculations depending on the reaction dynamics and equilibrium expressions.
Transcribed Image Text:**Chemical Equilibrium Problem** **Scenario:** Suppose a 250. mL flask is filled with 1.2 mol of \(H_2\) and 0.90 mol of \(HI\). This reaction becomes possible: \[ H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \] **Instructions:** Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use \(x\) to stand for the unknown change in the molarity of \(I_2\). You can leave out the \(M\) symbol for molarity. **Table Descriptions:** | | \(H_2\) | \(I_2\) | \(HI\) | |----------|---------|---------|--------| | initial | 1.2 | | | | change | | \(x\) | | | equilibrium | | | | - **Initial Molarity Row:** This row lists the initial molarity of the reactants and products before the reaction starts. According to the given problem, the initial molarity of \(H_2\) is 1.2 M. - **Change in Molarity Row:** This row represents the change in concentration of each species as the reaction progresses towards equilibrium. The change in molarity of \(I_2\) is represented by \(x\). - **Equilibrium Molarity Row:** This row shows the concentrations of reactants and products once the equilibrium is achieved. These need to be calculated based on the initial conditions and the change in molarity \(x\). Remember, the values in the table are intended to be filled out with specific calculations depending on the reaction dynamics and equilibrium expressions.
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