Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3.

(A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius.

(B) What will be the new equilibrium concentrations if the volume of the system is suddenly increased to 3.00 L at 25 degrees celcius.

(C) What effect would increasing the pressure at 25 degrees celcius have on the equilibrium?

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To answer these questions, we need to use the given equilibrium constant (Kc) and the stoichiometry of the reaction. The equilibrium constant expression is written as:

Kc = [NO2]^2 / [N2O4]

(A) To calculate the equilibrium concentrations, we need to use stoichiometry and the given mass of N2O4. First, we convert the mass of N2O4 to the number of moles using its molar mass. The molar mass of N2O4 is 92.02 g/mol.

Number of moles of N2O4 = 4.00 g / 92.02 g/mol = 0.04348 mol

Since the initial volume is 2.00 L, we can calculate the initial concentration of N2O4:

Initial concentration of N2O4 = number of moles / volume = 0.04348 mol / 2.00 L = 0.0217 M

Using the stoichiometry of the reaction, we know that every 1 mole of N2O4 produces 2 moles of NO2. Therefore, the initial concentration of NO2 is 0 M.

(B) When the volume of the system is suddenly increased to 3.00 L, the concentrations of both N2O4 and NO2 will change. However, since the volume increases, the number of moles of each gas remains constant.

The new concentration of N2O4 can be calculated using the new volume:

New concentration of N2O4 = number of moles / new volume = 0.04348 mol / 3.00 L = 0.0145 M

Using the stoichiometry of the reaction, the new concentration of NO2 can be found by multiplying the new concentration of N2O4 by 2:

New concentration of NO2 = 2 * new concentration of N2O4 = 2 * 0.0145 M = 0.029 M

(C) Increasing the pressure would shift the equilibrium toward the side with fewer gas molecules. In this case, there are fewer moles of gas on the reactant (N2O4) side compared to the product (NO2) side. Therefore, increasing the pressure would favor the formation of more gas molecules and shift the equilibrium towards the product side, resulting in an increase in the concentration of NO2.