to determined pseudo first order i follow this equation log(qe-qt)=log qe-k1t/2.303 but i found qe is lower than qt what can i do to plot log(qe-qt) versus t?
I assume q is heat release and qe is heat release at equilibrium and you are using q as a proxy for extent of reaction at isothermal condtiond. I don't know if your reaction is exothermic or endothermic but it appears you have a sign error and you should be plottng log(qt-qe) instead of Log(qe-qt). The 2.303 in your expression is is Ln(10) it is used to convert Loq to Ln. If you plot Ln(qt-qe) instead of Log(qt-qe)you will not need the 2.303 term.
Maybe qe and qt should be summed over the reaction time. Then reaction could be proceeding backward, or the reaction might be endothermic.
In this equation, qe is the adsorption capacity at equilibrium (mg g-1), qt is the adsorption capacity at time t (mg g-1) and k1 is the pseudo-first-order rate constant (min-1). It is impossible qe be lower than qt. Because in the adsorption process qt final reaches to qe. I think you have a mistake in the determination of qe.
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