What do we know?What do we know? Direction of reaction to shift for equilibrium NEED TO KNOW: quantify amount of reactants and products at equilibrium.
Using K C to determine [products] and [reactants] at equilibrium Only know K C and initial concentrations of reactants Changes in concentration of chemical compounds ( Δ C) Related to STOICHIOMETRIC ratios in chemical equation. Represents concentration change from initial to equilibrium conditions.
Example 1Example 1 2H 2 + O 2 2H 2 O So what is [H 2 ] at equilibrium? [H 2 ] at equilibrium = [H 2 ] initial – Δ H 2 **Use stoichiometric ratios to determine the amount of Δ C**
Example 2:Example 2: 1 mole of butane is in a 1L flask at 25°C with no isobutane present. What will be the equilibrium concentrations of butane and isobutane with a K C of 2.5 for this reaction?
Equilibrium Key Elements in Problem Balanced Equation Equilibrium constant Initial Conditions Problem’s Objective
Steps for Complex Problems 1)Decide if the reaction is at equilibrium 2)Set up equilibrium expression 3)Make an ICE Chart 4)Solve for Δ C 5)Is assumption valid for Δ C? 6)Determine the final concentrations of the chemical compounds.
Ice ChartIce Chart “ICE”ReactantsProducts Initial Concentrations (I): Change in Concentration ( Δ C or x): Equilibrium Concentrations (E):
Assumption with Δ CAssumption with Δ C If Δ C < 5% of initial concentration, ignore the Δ C for adding and subtracting in equilibrium expression. If Q< K, both small values so initial concentrations close to equilibrium Always validate this assumption in an equilibrium problem
Assumption with Δ C (cont.)Assumption with Δ C (cont.) If K eq < 1x10 -4, remove the “x or Δ C” value in denominator. Δ C is very small compared to initial concentration so subtraction would not be a huge difference. Only works when adding or subtracting Δ C If concentrations or partial pressures are very small where their magnitude is approximately equal to K eq, CANNOT discount Δ C value.
Example 3:Example 3: H 2 O (g) is present in a rigid container at 25°C with an initial partial pressure of atm. What are the partial pressures of H 2(g) and O 2(g) at equilibrium? (K P = 2.0 x )
Example 3: continuedExample 3: continued
Example 4:Example 4: Sulfur trioxide decomposes to form sulfur dioxide and oxygen at 300°C°. Calculate the concentrations of all chemical compounds at equilibrium with an initial SO 3 concentration of 0.100M and K C = 1.6 x
Example 4: continuedExample 4: continued
Example 5:Example 5: mol of COCl 2 comes to equilibrium in a 5.8L container at 25°C (K C = 7.27 x ). Find the equilibrium concentrations of all chemical compounds in the following equation. ( Hint: first find the initial [COCl 2 ] ) COCl 2 (g) CO (g) + Cl 2 (g)
Example 5: continuedExample 5: continued
In ClassIn Class Problems on Equilibrium II Worksheet
Homework AP Equilibrium and ICE method worksheet (#1-5)