WARM UP 2.00 moles of NOCl was placed in a 2.00 liter reaction vessel at 400°C. After equilibrium was established, it was found that 24% of the NOCl had.

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WARM UP 2.00 moles of NOCl was placed in a 2.00 liter reaction vessel at 400°C. After equilibrium was established, it was found that 24% of the NOCl had dissociated according to the following equation: 2NOCl(g) 2NO(g) + Cl2(g). Calculate the equilibrium constant, K, for the reaction.

Predicting Equilibrium

Calculating Concentrations Use K and initial concentrations to determine the concentrations at equilibrium N2O4 2NO2 K = .00463 2.5 moles N2O4 1 L container

Calculating Concentrations Set up an ICE table Make x the change N2O4 2NO2 Initial 2.5 0 Change - x + 2x Equilibrium 2.5 – x 2x

Calculating Concentrations 2. Write the equilibrium constant expression and solve for x .00463 = [2x]2 [2.5 – x]

Calculating Concentrations May need to create quadratic equation ax2 + bx + c Use formula to solve for x -4x2 - .00463x + .011575 x = .053

Calculating Concentrations 3. Plug x into concentration values at equilibrium for all molecules x = .053 N2O4 (2.5 - .053) = 2.447 NO2 = 2(.053) = .106

WRAP UP Calculate the concentration of OH- ions present after 2.7 M of the weak base, QOH (the reactant), is allowed to dissociate into its Q+ and OH- product ions. The Kb value for this process is 8.3 x 10-2.