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Unformatted text preview: efficients of equation 1 are twice those of equation 2, K for equation 1 is the square of that for equation 2. EXAMPLE Equation 1: Equation 2:
K2 Q HI2 2x 2 2x 2 K 55.64 H2 I2 2.00 x 2.00 x 2.00 x 2 C(s) + ½ O2 (g) ⇌ CO (g) 2 C(s) + O2 (g) ⇌ 2 CO (g) C(s) CO (g) CO 2 K1 1/ 2 O2 2 x 1.58 mol L-1 H2 I2 2.00 mol L-1 1.58 mol L-1 0.42 mol L-1 CO2 O2 HI 2 1.58 mol L-1 3.16 mol L-1 4 Reaction Equations and Equilibrium Constants Reaction Equations and Equilibrium Constants Reversing the Reaction Equation
If the equation for an equilibrium reaction is the reverse of another, K for each reaction is the reciprocal of the other. EXAMPLE Equation 1: HCOOH (aq) + H2O(l) ⇌ HCOO- (aq) + H3O- (aq) Equation 2: HCOO- (aq) + H3O- (aq) ⇌ HCOOH (aq) + H2O(l)
K1 Deriving an Equilibrium Constant from Others
Dissolving solid silver chloride by adding ammonia. (Left) A precipitate of AgCl(s) is suspended in water. (Right) When a concentrated solution of ammonia is added, the ammonia reacts with the low level of Ag+(aq) ions in solution to form [Ag(NH3)2]+ complex ions. HCOO H O...
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- Spring '11