{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

5 chemistry102 chapter14 equilibriumconstant

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: elementary reactions. At Equilibrium: Rate (forward reaction) = Rate(reverse reaction) 2 kf [N2O4] = kr [NO2] k f [NO 2 ]2 = = constant k r [N 2O 4 ] k f = K c = equilib rium con stant k r implies mo lar concentration In General: aA + bB K c = ¾¾ ® ¬¾ ¾ cC + dD d [C]c [D] [A]a [B]b [C], [D] = mo lar concentrations (mo larit ies) of the products at equilibrium [A], [B] = mo lar concentrations (mo larit ies) of the reactants at equilibrium · This relat ionship was postulated by two chemists in 1864 and called the law of mass action. 5 Chemistry 102 Chapter 14 EQUILIBRIUM CONSTANT · The Equilibrium Constant, Kc, is a constant for a particular reaction at a given temperature. NOTE: 1. If the overall react ion occurs by a mult i­step mechanism, one can show that Kc for the overall reaction equals a product of ratios of the individual rate constants. 2. It is co mmo n practice to write Kc wit hout units Example 1: Write the equilibrium constant expressio n for the equation shown below: ¾¾ ® 2 NO2 (g) + 7 H2 (g) ¬¾ 2 NH3 (g) + 4 H2O(...
View Full Document

{[ snackBarMessage ]}

Ask a homework question - tutors are online