Three experiments were run starting with different initial amounts of N_2O_4(g)
ID: 497846 • Letter: T
Question
Three experiments were run starting with different initial amounts of N_2O_4(g) ([N_2O_4]_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 ([NO_2]^2/(N_2O_4]) is equal to a constant value. Each experiment reached a different set of equilibrium concentrations.Explanation / Answer
1. True - Each experiment started with a different initial concentration of N2O4
2. False- the ratio([NO2]/N2O4]) is equal to a constant value
3.False- the ratio(2*[NO2]/N2O4]) is equal to a constant value
4.True- the ratio([NO2]2/N2O4]) is equal to a constant value
5. True- Each experiment reached a disfferent set of equilibrium concentrations
exp [N2O4]0 [NO2] [N2O4] [NO2]/N2O4] 2[NO2]/[N2O4] [NO2]2/[N2O4} 1 3.5 2.85 2.1 1.35 2.7 3.86 2 3.1 2.64 1.8 1.47 2.94 3.87 3 2.6 2.33 1.4 1.66 3.32 3.87