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. [NO₂] / [N₂04] Exp [N₂0410 [NO₂] [N₂04] 2.98 2.3 2.64 1.8 2.06 1.1 1 2 3 3.8 3.1 2.1 2 [NO₂] / [NO₂]²/ [N₂04] [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. W Previous Next

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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.
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 N₂O4 at equilibrium.
Be sure to round to the correct number of significant figures.
[NO₂] /
[N₂04]
Exp[N204]0[NO₂] [N₂04]
1
2
3
3.8
3.1
2.1
2.98 2.3
2.64 1.8
2.06 1.1
2 [NO₂] / [NO₂]²/
[N₂04] [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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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) ([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. [NO₂] / [N₂04] Exp[N204]0[NO₂] [N₂04] 1 2 3 3.8 3.1 2.1 2.98 2.3 2.64 1.8 2.06 1.1 2 [NO₂] / [NO₂]²/ [N₂04] [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. Previous Next
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