Three experiments were run starting with different initial amounts of N_2O_4l_0

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.

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