TS 385 GENERAL CHEMISTRY STUDY SHEET NO. 25 1. Write the equation relating K, to

Question

TS 385 GENERAL CHEMISTRY STUDY SHEET NO. 25 1. Write the equation relating K, to molarities of reactants and products for each of the following equilibrium reactions. 2. For the reaction N2O4 (g)2NO2(g), the equilibrium constant is 0.00576 at 25°C. If 0.000500 mol of N204 are added to a 2.00 L flask of 25°C allowed to come to equilibrium, what are the equilibrium molarities of N204 and NO2? 3. Which of the following would have to be solved using the quadratic equation? a. For the equilibrium of AP (APA+P), calculate the molarity of A if the initial molarity of AP 0.30 and K 0.00039 b. For the equilibrium of MD (MD M+ D), calculate the molarity of D ift initial molarity of MD 0.25 and K 0.015. For the equilibrium of XY X+Y XY), calculate the molarity of X, if

Explanation / Answer

Initial Molarity of N2O4 = Number of moles added/Volume of flask = 0.000500/2 = 0.000250M

N2O4(g) ======= 2NO2(g)

0.000250 0

0.000250-x 2x

K = [Products]/[Reactants] = (2x)^2/(0.000250-x) = 0.00576

solving the quadratic equation we get

x = 0.000217

Equilibrium molarity of NO2 = 2x = 2(0.000217) = 0.000434M

Equilibrium molarity of N2O4 = 0.000250 - x = 0.000250 - 0.000217= 0.000033M

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