Mayo–Lewis equation

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The Mayo–Lewis equation or copolymer equation in polymer chemistry describes the distribution of monomers in a copolymer:^[1] It is named for Frank R. Mayo and Frederick M. Lewis.

Taking into consideration a monomer mix of two components $M_1\,$ and $M_2\,$ and the four different reactions that can take place at the reactive chain end terminating in either monomer ( $M^*\,$ ) with their reaction rate constants $k\,$ :

$M_1^* + M_1 \xrightarrow{k_{11}} M_1M_1^* \,$

$M_1^* + M_2 \xrightarrow{k_{12}} M_1M_2^* \,$

$M_2^* + M_2 \xrightarrow{k_{22}} M_2M_2^* \,$

$M_2^* + M_1 \xrightarrow{k_{21}} M_2M_1^* \,$

and with reactivity ratios defined as:

$r_1 = \frac{k_{11}}{k_{12}} \,$

$r_2 = \frac{k_{22}}{k_{21}} \,$

the copolymer equation is given as:

$\frac {d\left [M_1 \right]}{d\left [M_2\right]}=\frac{\left [M_1\right]\left (r_1\left[M_1\right]+\left [M_2\right]\right)}{\left [M_2\right]\left (\left [M_1\right]+r_2\left [M_2\right]\right)}$

with the concentration of the components given in square brackets. The equation gives the copolymer composition at any instant during the polymerization.

Limiting cases

From this equation several limiting cases can be derived:

$r_1 = r_2 >> 1 \,$ with both reactivity ratios very high the two monomers have no inclination to react to each other except with themselves leading to a mixture of two homopolymers.
$r_1 = r_2 > 1 \,$ with both ratios larger than 1, homopolymerization of component M_1 is favored but in the event of a crosspolymerization by M_2 the chain-end will continue as such giving rise to block copolymer
$r_1 = r_2 \approx 1 \,$ with both ratios around 1, monomer 1 will react as fast with another monomer 1 or monomer 2 and a random copolymer results.
$r_1 = r_2 \approx 0 \,$ with both values approaching 0 the monomers are unable to react in homopolymerization and the result is an alternating polymer
$r_1 >> 1 >> r_2 \,$ In the initial stage of the copolymerization monomer 1 is incorporated faster and the copolymer is rich in monomer 1. When this monomer gets depleted, more monomer 2 segments are added. This is called composition drift.

An example is maleic anhydride and stilbene, with reactivity ratio:

Maleic anhydride ( $r_1\,$ = 0.08) & cis-stilbene ( $r_2 ,$ = 0.07)
Maleic anhydride ( $r_1\,$ = 0.03) & trans-stilbene ( $r_2 ,$ = 0.03)

Both of these compounds do not homopolymerize and instead, they react together to give exclusively alternating copolymer.

Another form of the equation is:

$F_1=1-F_2=\frac{r_1 f_1^2+f_1 f_2}{r_1 f_1^2+2f_1 f_2+r_2f_2^2}\,$

where $F\,$ stands the mole fraction of each monomer in the copolymer:

$F_1 = 1 - F_2 = \frac{d M_1}{d (M_1 + M_2)} \,$

and $f\,$ the mole fraction of each monomer in the feed:

$f_1 = 1 - f_2 = \frac{M_1}{(M_1 + M_2)} \,$

When the copolymer composition has the same composition as the feed, this composition is called the azeotrope.

Calculation of reactivity ratios

The reactivity ratios can be obtained by rewriting the copolymer equation to:

$\frac{f(1-F)}{F} = r_2 - r_1\left(\frac{f^2}{F}\right) \,$

with

$f = \frac{[M_1]}{[M_2]} \,$ in the feed

and

$F = \frac{d[M_1]}{d[M_2]} \,$ in the copolymer

A number of copolymerization experiments are conducted with varying monomer ratios and the copolymer composition is analysed at low conversion. A plot of $\frac{f(1-F)}{F}\,$ versus $\frac{f^2}{F}\,$ gives a straight line with slope $r_1\,$ and intercept $r_2\,$ .

A semi-empirical method for the determination of reactivity ratios is called the Q-e scheme.

Equation derivation

Monomer 1 is consumed with reaction rate:^[2]

$\frac{-d[M_1]}{dt} = k_{11}[M_1]\sum[M_1^*] + k_{21}[M_1]\sum[M_2^*] \,$

with $\sum[M_x^*]$ the concentration of all the active centers terminating in monomer 1 or 2.

Likewise the rate of disappearance for monomer 2 is:

$\frac{-d[M_2]}{dt} = k_{12}[M_2]\sum[M_1^*] + k_{22}[M_2]\sum[M_2^*] \,$

Division of both equations yields:

$\frac{d[M_1]}{d[M_2]} = \frac{[M_1]}{[M_2]} \left( \frac{k_{11}\frac{\sum[M_1^*]}{\sum[M_2^*]} + k_{21}} {k_{12}\frac{\sum[M_1^*]}{\sum[M_2^*]} + k_{22}} \right) \,$

The ratio of active center concentrations can be found assuming steady state with:

$\frac{d\sum[M_1^*]}{dt} = \frac{d\sum[M_2^*]}{dt} \approx 0\,$

meaning that the concentration of active centres remains constant, the rate of formation for active center of monomer 1 is equal to the rate of their destruction or:

$k_{21}[M_1]\sum[M_2^*] = k_{12}[M_2]\sum[M_1^*] \,$

$\frac{\sum[M_1^*]}{\sum[M_2^*]} = \frac{k_{21}[M_1]}{k_{12}[M_2]}\,$

External links

copolymer equation applet @eng.utah.edu Link
copolymers @zeus.plmsc.psu.edu Link

References

↑ Copolymerization. I. A Basis for Comparing the Behavior of Monomers in Copolymerization; The Copolymerization of Styrene and Methyl Methacrylate Frank R. Mayo and Frederick M. Lewis J. Am. Chem. Soc.; 1944; 66(9) pp 1594 - 1601; doi:10.1021/ja01237a052
↑ Young, Robert J. (1983). Introduction to polymers ([Reprinted with additional material] ed.). London: Chapman and Hall. ISBN 0-412-22170-5.

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