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Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(g) = 2NO(3) 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 N,. You can leave out the M symbol for molarity. N2 02 NO initial change equilibrium

Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(g) = 2NO(3) 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 N,. You can leave out the M symbol for molarity. N2 02 NO initial change equilibrium

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Suppose a 500. mL flask is filled with 1.4 mol of N₂ and 1.3 mol of NO. This reaction becomes possible: \[ \text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g) \] 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 \( \text{N}_2 \). You can leave out the \( M \) symbol for molarity. | | \( \text{N}_2 \) | \( \text{O}_2 \) | \( \text{NO} \) | |----------|------------|------------|---------| | initial | | | | | change | \( x \) | | | | equilibrium | | | |
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.4 mol of N₂ and 1.3 mol of NO. This reaction becomes possible: \[ \text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g) \] 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 \( \text{N}_2 \). You can leave out the \( M \) symbol for molarity. | | \( \text{N}_2 \) | \( \text{O}_2 \) | \( \text{NO} \) | |----------|------------|------------|---------| | initial | | | | | change | \( x \) | | | | equilibrium | | | |
Expert Solution
Step 1

Given:

Initial moles of N2 = 1.4 mol

Initial moles of NO = 1.3 mol

Volume of flask = 500.0 mL = 0.5 L

 

Note: initial moles of O2 is not given, so we are considering concentration of O2 as "y"

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