I HAVE TO FILL IN THE BOX AND ANSWER THE TRUE/FALSE TO COMPLETE THE PROBLEM
1a. Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas.
N2O4(g) ------> 2 NO2(g) |
Three experiments were run starting with different initial amounts
of N2O4(g)
([N2O4]0 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 | [N2O4]0 | [NO2] | [N2O4] | [NO2] / [N2O4] | 2 [NO2] / [N2O4] | [NO2]2 / [N2O4] | ||||
1 | 3.7 | 2.92 | 2.2 | |||||||
2 | 3.1 | 2.64 | 1.8 | |||||||
3 | 2.1 | 2.06 | 1.1 |
Based on your calculations, indicate whether each statement is
True (T) or False (F):
___TF1. Each experiment started with a different
initial concentration of N2O4.
___TF2. The ratio ([NO2] /
[N2O4]) is equal to a constant value.
___TF3. The ratio (2 [NO2] /
[N2O4]) is equal to a constant value.
___TF4. The ratio ([NO2]2 /
[N2O4]) is equal to a constant value.
___TF5. Each experiment reached a different set of
equilibrium concentrations.
1b. 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 | [N2O4]0 | [NO2] | [N2O4] | [NO2] / [N2O4] | 2 [NO2] / [N2O4] | [NO2]2 / [N2O4] | ||||
1 | 3.7 | 2.92 | 2.2 | |||||||
2 | 3.1 | 2.64 | 1.8 | |||||||
3 | 2.3 | 2.15 | 1.2 |
Based on your calculations, indicate whether each statement is
True (T) or False (F):
___TF1. Each experiment started with a different
initial concentration of N2O4.
___TF2. The ratio ([NO2] /
[N2O4]) is equal to a constant value.
___TF3. The ratio (2 [NO2] /
[N2O4]) is equal to a constant value.
___TF4. The ratio ([NO2]2 /
[N2O4]) is equal to a constant value.
___TF5. Each experiment reached a different set of
equilibrium concentrations.
Based on your calculations, indicate whether each statement is
True (T) or False (F):
___TF1. Each experiment started with a different
initial concentration of N2O4.= True
(T)
___TF2. The ratio ([NO2] /
[N2O4]) is equal to a constant value.=
False (F):
___TF3. The ratio (2 [NO2] /
[N2O4]) is equal to a constant value. =
False (F):
___TF4. The ratio ([NO2]2 /
[N2O4]) is equal to a constant value. =
True (T)
___TF5. Each experiment reached a different set of
equilibrium concentrations.= False (F):
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