At 100 °C, Kc = 4.72 for the reaction 2 NO21g2 ∆ N2O41g2. An empt...

Question

At 100 °C, Kc = 4.72 for the reaction 2 NO21g2 ∆ N2O41g2. An empty 10.0-L flask is filled with 4.60 g of NO2 at 100 °C. What is the total pressure in the flask at equilibrium?

Accepted Answer

Calculate the number of moles of NO2 initially present using the molar mass of NO2. The molar mass of NO2 is approximately 46.0 g/mol.. Use the ideal gas law to calculate the initial pressure of NO2 in the flask. The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.. Set up the ICE table (Initial, Change, Equilibrium) for the reaction: 2 NO2(g) ⇌ N2O4(g). Fill in the initial concentrations, the change in concentrations as the reaction proceeds towards equilibrium, and the equilibrium concentrations.. Write the expression for the equilibrium constant Kc and substitute the equilibrium concentrations from the ICE table. Solve for the unknowns, which represent the changes in concentration due to the reaction reaching equilibrium.. Calculate the total pressure at equilibrium by adding the partial pressures of NO2 and N2O4. Use the equilibrium concentrations and the ideal gas law to find the partial pressures.

At 100 °C, Kc = 4.72 for the reaction 2 NO21g2 ∆ N2O41g2. An empty 10.0-L flask is filled with 4.60 g of NO2 at 100 °C. What is the total pressure in the flask at equilibrium?

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Key Concepts

Equilibrium Constant (Kc)

Ideal Gas Law

Stoichiometry of Gaseous Reactions