Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N₂O4(9) ? 2 NO₂(g) Three experiments were run starting with different initial amounts of N₂O4(g) ([N₂O4lo 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 [N₂04]0 [NO₂] [N₂04] 1 3.8 2 3.1 3 2.1 2.98 2.3 2.64 1.8 2.06 1.1 [NO₂] 2 [NO₂] [N₂04] / [N₂04] [NO₂]² [N₂04] 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] / [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.
Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N₂O4(9) ? 2 NO₂(g) Three experiments were run starting with different initial amounts of N₂O4(g) ([N₂O4lo 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 [N₂04]0 [NO₂] [N₂04] 1 3.8 2 3.1 3 2.1 2.98 2.3 2.64 1.8 2.06 1.1 [NO₂] 2 [NO₂] [N₂04] / [N₂04] [NO₂]² [N₂04] 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] / [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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Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....
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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.
N₂04(9) 2 NO₂(g)
Three experiments were run starting with different initial
amounts of N₂O4(g) ([N2O4lo 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.
1
2
3
Exp [N₂04]0 [NO₂] [N₂04]
3.8
3.1
2.1
2.98 2.3
2.64 1.8
2.06 1.1
[NO₂] / 2 [NO₂]
[N₂04] / [N₂04]
[NO₂]²
[N₂04]
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] / [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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2c1d2e3-89ea-47de-ad2a-ad4f6e93129c%2F018a07ad-2e89-4d3b-929c-a71c54063c06%2Fo8p70vt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Dinitrogen tetraoxide is a colorless gas at room temperature. It
can dissociate into nitrogen dioxide, which is a reddish brown
gas.
N₂04(9) 2 NO₂(g)
Three experiments were run starting with different initial
amounts of N₂O4(g) ([N2O4lo 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.
1
2
3
Exp [N₂04]0 [NO₂] [N₂04]
3.8
3.1
2.1
2.98 2.3
2.64 1.8
2.06 1.1
[NO₂] / 2 [NO₂]
[N₂04] / [N₂04]
[NO₂]²
[N₂04]
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] / [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.
![Dinitrogen tetraoxide is a colorless gas at room temperature. It
can dissociate into nitrogen dioxide, which is a reddish brown
gas.
N₂O4(9) 2 NO₂(g)
Three experiments were run starting with different initial
amounts of N₂O4(g) ([N₂O4]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]
1
2
3
3.8
3.0
2.4
2.98 2.3
2.56 1.7
2.24 1.3
[NO₂] 2 [NO₂]
[N2₂04] / [N₂04]
[NO₂]2
[N₂04]
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] / [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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2c1d2e3-89ea-47de-ad2a-ad4f6e93129c%2F018a07ad-2e89-4d3b-929c-a71c54063c06%2F7gyzogd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Dinitrogen tetraoxide is a colorless gas at room temperature. It
can dissociate into nitrogen dioxide, which is a reddish brown
gas.
N₂O4(9) 2 NO₂(g)
Three experiments were run starting with different initial
amounts of N₂O4(g) ([N₂O4]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]
1
2
3
3.8
3.0
2.4
2.98 2.3
2.56 1.7
2.24 1.3
[NO₂] 2 [NO₂]
[N2₂04] / [N₂04]
[NO₂]2
[N₂04]
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] / [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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