- equilibrium in reactions when forward/reverse reactions occur at same rate ratio of partial pressures concentrations equals constant pressures

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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.

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