Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N204. 2. The ratio ([NO2] / [N2O4]) is equal to a constant value. 3. The ratio (2 [NO2] / [N2O4]) is equal to a constant value. 4. The ratio ([NO2]² / [N2O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.
Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N204. 2. The ratio ([NO2] / [N2O4]) is equal to a constant value. 3. The ratio (2 [NO2] / [N2O4]) is equal to a constant value. 4. The ratio ([NO2]² / [N2O4]) is equal to a constant value. 5. Each experiment reached a different set of equilibrium concentrations.
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Chapter21: Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 21.200QP
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Question
![N204(g) = 2 NO2(g)
Three experiments were run starting with different initial amounts of N2O4(g) ([N204]o 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 NO2 and N204 at equilibrium.
Be sure to round to the correct number of significant figures.
Exp[N204l0 [NO2][N,04] [NO,] / [N204] 2 [NO,] / [N204] [NO2]? / [N204]
1
3.7
2.92
2.2
2
3.0
2.56 1.7
3
2.3
2.15
1.2
Based on your calculations, indicate whether each statement is True (T) or False (F):
v1. Each experiment started with a different initial concentration of N204.
v2. The ratio ([NO2] / [N204]) is equal to a constant value.
v3. The ratio (2 [NO2] / [N204]) is equal to a constant value.
v 4. The ratio ([NO2]? / [N204]) is equal to a constant value.
v5. Each experiment reached a different set of equilibrium concentrations.
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Transcribed Image Text:N204(g) = 2 NO2(g)
Three experiments were run starting with different initial amounts of N2O4(g) ([N204]o 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 NO2 and N204 at equilibrium.
Be sure to round to the correct number of significant figures.
Exp[N204l0 [NO2][N,04] [NO,] / [N204] 2 [NO,] / [N204] [NO2]? / [N204]
1
3.7
2.92
2.2
2
3.0
2.56 1.7
3
2.3
2.15
1.2
Based on your calculations, indicate whether each statement is True (T) or False (F):
v1. Each experiment started with a different initial concentration of N204.
v2. The ratio ([NO2] / [N204]) is equal to a constant value.
v3. The ratio (2 [NO2] / [N204]) is equal to a constant value.
v 4. The ratio ([NO2]? / [N204]) is equal to a constant value.
v5. Each experiment reached a different set of equilibrium concentrations.
(Previous
Next
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