Equations . . Zero Order Reactions Fig. .
: Variation in the concentration vs time plot for a zero order reaction Time k = -slope Concentration of R [R ] Comparing ( . ) with equation of a straight line, y = mx + c, if we plot [R] against t, we get a straight line (Fig. . ) with slope = – k and intercept equal to [R] .
Further simplifying equation ( . ), we get the rate constant, k as ( . ) Zero order reactions are relatively uncommon but they occur under special conditions. Some enzyme catalysed reactions and reactions which occur on metal surfaces are a few examples of zero order reactions.
The decomposition of gaseous ammonia on a hot platinum surface is a zero order reaction at high pressure.