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HW 4-Intro to Equilibrium

Microscopic Reversibility

2 Equilibrium Constant Mathemat...

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Question

3 Equilibrium Constant: Magnitude

4. Exploring Equilibrium: Nitrogen

5 Writing Equilibrium Expressions

6 Writing Equilibrium Expressions

7. Manipulating K Expressions

8 Calculate K for Rearranged Equ

9 Writing Equilibrium Expressions:

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Due Jun 22 at 11:55 PM

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Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas,

N₂O₂(9) 2 NO₂(g)

[Review Topics

References]

Use the References to access important values if needed for this question.

Three experiments were run starting with different initial amounts of N₂O.(g) (N₂Olo in the table). The systems were allowed to reach

equilibrium and the concentrations for each gas were measured (in units of moles/Liter).

For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists

between the concentrations of NO and N₂O4 at equilibrium.

Be sure to round to the correct number of significant figures.

Exp [N₂O4]o [NO₂] [N₂O₁] [NO₂] / [N₂O₁] 2 [NO₂] / [N,O₂] [NO,] / [N₂O₁]

1

3.5

2.85 2.1

2

3.1

2.64 1.8

2.6

2.33 1.4

3

Based on your calculations, indicate whether each statement is True (T) or False (F):

1. Each experiment started with a different initial concentration of N₂O

2. The ratio ([NO]/[NO]) is equal to a constant value.

3. The ratio (2 [NO₂1/[N₂O₂]) is equal to a constant value.

4. The ratio ([NO₂12/ [N₂O) is equal to a constant value.

5. Each experiment reached a different set of equilibrium concentrations.

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