Calculate Equilibrium Amount of NO₂ in a Reaction
What is the equilibrium constant, Kc, for the reaction N₂O₄(g) <--> 2 NO₂(g) at 25°C?
The equilibrium constant, Kc, for the reaction N₂O₄(g) <--> 2 NO₂(g) at 25°C is 170.
How much N₂O₄ is placed in a 5.000 L flask at 25°C?
15.6 g of N₂O₂ is placed in a 5.000 L flask at 25°C.
Calculate the amount of NO₂ (mol) present at equilibrium.
Final answer:
The amount of NO₂ (mol) present at equilibrium can be calculated using the given information about N₂O₄ and the equilibrium constant Kc.
To calculate the amount of NO₂ (mol) present at equilibrium, we need to first calculate the amount of N₂O₄ (mol) present. From the given data, we have 15.6 g of N₂O₄. We can calculate the amount of N₂O₄ (mol) by using its molar mass:
Molar mass of N₂O₄ = 92.015 g/mol
Amount of N₂O₄ (mol) = 15.6 g / 92.015 g/mol
Next, we can use the stoichiometric coefficients in the balanced equation to determine the amount of NO₂ (mol) at equilibrium. Since the stoichiometric coefficient of NO₂ is 2, the amount of NO₂ (mol) will be twice the amount of N₂O₄ (mol).
Amount of NO₂ (mol) = 2 * Amount of N₂O₄ (mol)
By following these steps, we can calculate the amount of NO₂ (mol) present at equilibrium.