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If the concentration of a reactant remains constant (because it is a catalyst, or because it is in great excess with respect to the other reactants), its concentration can be included in the rate constant, leading to a pseudo–first-order (or occasionally pseudo–second-order) rate equation. For a typical second-order reaction with rate ...
In fact, however, the observed reaction rate is second-order in NO 2 and zero-order in CO, [5] with rate equation r = k[NO 2] 2. This suggests that the rate is determined by a step in which two NO 2 molecules react, with the CO molecule entering at another, faster, step. A possible mechanism in two elementary steps that explains the rate ...
For this reason, the Euler method is said to be a first-order method, while the midpoint method is second order. We can extrapolate from the above table that the step size needed to get an answer that is correct to three decimal places is approximately 0.00001, meaning that we need 400,000 steps.
Consider , the exact solution to a differential equation in an appropriate normed space (, | | | |). Consider a numerical approximation u h {\displaystyle u_{h}} , where h {\displaystyle h} is a parameter characterizing the approximation, such as the step size in a finite difference scheme or the diameter of the cells in a finite element method .
The steady-state rate equation is of mixed order and predicts that a unimolecular reaction can be of either first or second order, depending on which of the two terms in the denominator is larger. At sufficiently low pressures, k − 1 [ M ] ≪ k 2 {\displaystyle k_{-1}[{\ce {M}}]\ll k_{2}} so that d [ P ] / d t = k 1 [ A ] [ M ...
The rate of an S N 2 reaction is second order, as the rate-determining step depends on the nucleophile concentration, [Nu −] as well as the concentration of substrate, [RX]. [1] r = k[RX][Nu −] This is a key difference between the S N 1 and S N 2 mechanisms.
In chemistry, the effective molarity (denoted EM) [1] is defined as the ratio between the first-order rate constant of an intramolecular reaction and the second-order rate constant of the corresponding intermolecular reaction (kinetic effective molarity) [1] [2] or the ratio between the equilibrium constant of an intramolecular reaction and the equilibrium constant of the corresponding ...
Plugging in the first CSTR equation to the second: = (+) Therefore for m identical CSTRs in series: C A m = C A o ( 1 + k τ ) m {\displaystyle C_{Am}={\frac {C_{Ao}}{(1+k\tau )^{m}}}} When the volumes of the individual CSTRs in series vary, the order of the CSTRs does not change the overall conversion for a first order reaction as long as the ...