equilibrium in reactions - when forward/reverse reactions occur at same rate • ratio of partial pressures, concentrations equals constant • pressures no longer change • reaction continues to occur, but ratio stays the same (no net change) • can be reached from either direction Haber Process - synthesizing ammonia from hydrogen/nitrogen • world’s main source for fixed nitrogen • N2 + 3H2 <<>> 2NH3 equilibrium constant - only changed by temperature, not by reaction mechanism • for reaction aA + bB <<>> cC + dD • Keq = (C concentration)c(D concentration)d / (A concentration)a(B concentration)b • value determined by coefficients in chemical equation • value greater than 1 >> equilibrium towards product side • value less than 1 >> equilibrium towards reactant side • for any reaction, constant equal to reciprocal of constant for reverse reaction •
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This document was uploaded on 10/30/2011 for the course CHEM 161 at Rutgers.