Three experiments were run starting with different initial amounts of N_2O_4l_0
ID: 497845 • Letter: T
Question
Three experiments were run starting with different initial amounts of N_2O_4l_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 NO_2 and N_2O_4 at equilibrium. Based on your calculations, indicate whether each statement is True (T) or False (F): Each experiment started with a different initial concentration of N_2O_4. the ratio ([NO_2)/[N_2O_4]) is equal to a constant value. the ratio (2 [NO_2]/[N_2O_4]) is equal to a constant value. the ratio ([NC_2]^2/[N_2O_4]) is equal to a constant value. Each experiment reached a different set of equilibrium concentrations.Explanation / Answer
For the given reaction,
Data table
Exp [NO2]/[N2O4] 2[NO2]/[N2O4] [NO2]^2/[N2O4]
1 1.360 2.714 3.868
2 1.506 3.012 3.855
3 1.792 3.584 3.852
Based on the calculations, True/False statement
True : 1. Each experiment started with a different initial concentration of N2O4
False : 2. The ratio of ([NO2]/[N2O4]) is equal to a constant value.
False : 3. The ratio of (2[NO2]/[N2O4]) is equal to a constant value.
True : 4. The ratio of ([NO2]^2/[N2O4]) is equal to a constant value.
True : 5. Each experiment reached a different set of equilibrium concentrations.