Question

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).
1. For each of 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 3.0 2.56 1.7
3 2.1 2.06 1.1
2. 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.

Answer 1

Complete Question

The complete question is shown on the first uploaded image

Answer:

The calculation and filling of the table based on the ratio indicated by the column is shown on the second uploaded image

1 This is True

2 This is False

3 This is False

4 This is  True

5 This is  True

Explanation:

Based on your calculations, indicate whether each statement is True (T) or False (F):

Considering the first statement

Looking at the question we can see that the first statement is TRUE this because  all the three experiment have different initial concentration (3.5,3.0 & 2.6)

Considering the second  statement

 Looking at table we can see that the second statement is FALSE  because  

the ratio value of [NO2]/ [N2O4] in all three experiment have different value  1.4 , 1.5 & 1.7 is not a constant value.

Considering the Third  statement

Looking at the table we can see that the third statement is FALSE this  is because the ratio value of 2[NO2]/ [N2O4] in all three experiment have different value 2.7, 3.0 & 3.3 is not a constant value.

Considering the Fourth  statement

Looking at table we can see that the fourth statement is TRUE this is because the ratio value of$[NO2]^{2}/ [N2O4]$ in all three experiment have same value 3.9, 3.9 & 3.9 is a constant value.

Considering the Fifth  statement

Looking at table we can see that the fifth statement is TRUE this is because

each having different set of Equilibrium concentration