Ch 6_completed Pt 1 and 2_021712

# Ch 6_completed Pt 1 and 2_021712 - The Equilibrium Constant...

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The equilibrium constant is then expressed as a ratio of activities of products versus reactants as follows: This definition of the equilibrium constant supersedes the definition provided by Zumdahl in Section 6.2. The definition results in K being unitless, as it should! (Zumdahl only uses units in Ch 6 and calls them “apparent units.”) The Equilibrium Constant bB + cC ↔ dD + eE ° = ± ? ² ± ? ³ ± ? ´ ± ? µ

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Notice the effect of dividing by a standard (reference) state is to render each component of K unitless. The Equilibrium Constant (cont’d.) ° ? = ± NH 3 2 ± N ² ± H ² ³ = nh ³ 1 M 2 n 2 1 M h 2 1 M ³ K c = ´.1 × 10 −2 M 1 M 2 8.5 × 10 −µ M 1 M ´.1 × 10 −³ M 1 M ³ = ´.8 × 10 4
What if we multiply all the stoichiometric coefficients by 2? Still at equilibrium: [NH 3 ] = 3.1 x 10 -2 M, [N 2 ] = 8.5 x 10 -1 M, and [H 2 ] = 3.1 x 10 -3 M. What is the equilibrium constant? Multiply the coefficients by a constant, you raise the equilibrium constant to the power of the multiplier. The Equilibrium Constant (cont’d.) 2 N ± (g) + 6 H ± (g) ↔ 4 NH 3 (g) ° ? ′′ =

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Properties of the equilibrium constant: o K for a reaction written in reverse is the reciprocal of the original K expression: K new = ( K original ) -1 o If you multiply a chemical equation by a factor, n, the new
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Ch 6_completed Pt 1 and 2_021712 - The Equilibrium Constant...

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