N₂04(9) 2 NO₂(9) Three experiments were run starting with different initial amounts of N₂04(9) ([N20430 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 N₂O4 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N204]0 [NO2] [N₂04] [NO₂] / [N204] 2 [NO₂] / [N204] [NO₂]2/[N₂04] 1 2.92 2.2 1.3 2.56 1.7 1.5 2.06 1.1 2 3 3.7 3.0 2.1 2.65 3.01 3.8 3.8 Numeric input field 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..
N₂04(9) 2 NO₂(9) Three experiments were run starting with different initial amounts of N₂04(9) ([N20430 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 N₂O4 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N204]0 [NO2] [N₂04] [NO₂] / [N204] 2 [NO₂] / [N204] [NO₂]2/[N₂04] 1 2.92 2.2 1.3 2.56 1.7 1.5 2.06 1.1 2 3 3.7 3.0 2.1 2.65 3.01 3.8 3.8 Numeric input field 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..
Introductory Chemistry: A Foundation
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Author:Steven S. Zumdahl, Donald J. DeCoste
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Chapter17: Equilibrium
Section: Chapter Questions
Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...
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![N₂04(9) 2 NO₂(g)
Three experiments were run starting with different initial amounts of N₂04(9) ([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 N₂O4 at equilibrium.
Be sure to round to the correct number of significant figures.
Exp [N₂04]0 [NO₂] [N₂04] [NO₂] / [N₂04] 2 [NO₂] / [N204] [NO₂]2/[N₂04]
1
1.3
2.65
2.92 2.2
2.56 1.7
2
1.5
3.01
2.06 1.1
3
3.7
3.0
2.1
3.8
3.8 Numeric input field
Based on your calculations, indicate whether each statement is True (T) or False (F):
1. Each experiment started with a different initial concentration of N₂O4.
2. The ratio ([NO2] / [N₂04]) is equal to a constant value.
3. The ratio (2 [NO₂] / [N₂O4]) is equal to a constant value.
4. The ratio ([NO₂]2/[N₂04]) is equal to a constant value.
5. Each experiment reached a different set of equilibrium concentrations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd1f10484-52a0-4233-b031-0df053dd075b%2F6b4f06d1-e8b2-4021-bd3c-527758669c03%2Fd52tiyb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:N₂04(9) 2 NO₂(g)
Three experiments were run starting with different initial amounts of N₂04(9) ([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 N₂O4 at equilibrium.
Be sure to round to the correct number of significant figures.
Exp [N₂04]0 [NO₂] [N₂04] [NO₂] / [N₂04] 2 [NO₂] / [N204] [NO₂]2/[N₂04]
1
1.3
2.65
2.92 2.2
2.56 1.7
2
1.5
3.01
2.06 1.1
3
3.7
3.0
2.1
3.8
3.8 Numeric input field
Based on your calculations, indicate whether each statement is True (T) or False (F):
1. Each experiment started with a different initial concentration of N₂O4.
2. The ratio ([NO2] / [N₂04]) is equal to a constant value.
3. The ratio (2 [NO₂] / [N₂O4]) is equal to a constant value.
4. The ratio ([NO₂]2/[N₂04]) is equal to a constant value.
5. Each experiment reached a different set of equilibrium concentrations.
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