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Kinetics and Mechanism of Alkaline Hydrolysis of Urea and Sodium

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Kinetics and Mechanism of Alkaline Hydrolysis of Urea and Sodium Indian Journal of Chemistry Vol. 35A, December 1996, pp. 1116-1119 Kinetics and mechanism of alkaline formed during the hydrolysis of urea. Though the hydrolysis of urea and sodium cyanate mechanism had been given, neither rate determin- ing step had been defined nor rate expression had Zaheer Khan" been given. The alkaline hydrolysis of urea was Chemistry Department, Jamia Millia Islamia, not a simple first order reaction and required JamiaNagar, New Delhi 110 025, India much more kinetic studies. Therefore, the kinetics and of the reaction has been studied in alkaline medi- um with the aim to establish the consecutive na- MZ A Rafiquee, Kabir-ud-din, M Arif Niaz & A Aziz Khan ture as well as mechanism of two step hydrolysis Chemistry Department, AIigarh Muslim University, of urea. The rate constants of the consecutive AIigarh 202 002, India steps have been calculated using Swain equation". Received 20 March 1996; revised 20 June 1996 In support of the mechanism of ureolysis, basic The kinetics of hydrolysis of urea has been studied hydrolysis of cyante was also described in the in 0.5 to 3.0 mol dm - 3 sodium hydroxide solution at note. different temperatures. Urea hydrolysis follows an irreversible first order consecutive reaction path: Experimental Urea (BDH), sodium cyanate (Fluka) and sodi- 10bs 20bs um nitrate (E. Merck) were used as such. The • • urea k cyanate k NH3 + CO2 -NH3 stock solution of carbonate free sodium hydroxide (E. Merck) at about 17 mol dm "! was prepared The variation of k10bs with [alkali] is linear. at and diluted to the required concentrations using 3 [OH-]=5.0 to 1.5 mol dm- , thereafter a sharp in- doubly distilled water. All other reagents were of crease in the reaction rate is observed for first step reagent grade. Nessler's reagent was prepared by hydrolysis of urea. The second step rate constant literature method. (k )is found to be independent of [alkali].Hydroly- 2obS Hydrolysis of urea was carried out under two sis of urea in alkaline medium follows an elemination- addition mechanism. The reaction does not proceed different conditions. through the formation and decomposition of tetrahe- (i) Estimation of ammonia-A two-necked flask dral intermediate. Sodium cyanate hydrolysis obeys an containing sodium hydroxide and potassium nitr- irreversible pseudo-first order kinetics. [OH-] has no ate (used to maintain the ionic strength) was ther- significant effect on the rate constants. The following mostatted in an oil bath whose temperature was rate equations have been derived for the two step hy- maintained within ± 0.1"C. Urea solution was then drolysis of urea. added and the evolved ammonia was flushed' out by passing a continuous current of nitrogen gas and was absorbed in hydrochloric acid and then estimated at regular time intervals spectrophotom- etrically bynesslerization". k20bS = k2Kh (il) Estimation of unreacted [ureal-The con- On the basis of observed data, probable mechanisms centration of urea was estimated by taking out ali- have been proposed. quots at regular time intervals, neutralising it with standard acid solution after cooling, adding 4.0 ml Agriculture and biological importance of urea is of 50% H2S04 and 2.0 mi of working diacetyl well known. Hydrolysis of ureal occurs in acidic, monoxime solution in reaction after heating for neutral and alkaline media and in the presence of ten minutes in boiling water bath and measuring enzyme urease giving ammonia and carbondi- the absorbance of the developed pink colour at oxide. The hydrolysis of urea has been studied by 500 nm. Concentration of unreacted urea was es- Lynn? in 1.0 M to 2.0 M sodium hydroxide solu- timated from standard plot of absorbance versus tion, who showed that the basic ureolysis is a sim- urea solutions of known concentrations ranging ple pseudo-first order reaction. The concentration from 5.0 x 10-6 mol dm" to 35.0 x 10-6 mol of ammonia was estimated after a time sufficient dm - 3. This carbamido diacetyl reaction does not to allow the hydrolysis of any cyanate which give any colour with cyanate or ammonium ions. NOTES 1117 Table I-Activation parameters for the hydrolysis of urea and sodium cyanate ., Reaction so» sn» =ss» E. InA (.kJmol-l) (kf mol " '}(K-IJmol-l) (kJmol-l) (S-I) urea kIObSf'INC6 112.38 60.72 142.31 63.73 9.44 (110.00)(56.86) (146.39) (59.58)(8.94) NC6~NH3 108.01 52.53 153.41 55.34 8.09 (108.32) (49.67) (161.57) (52.68)(7.11) /j. C" calculated at 363K. Parantheses values are for the estimation of urea concentration and sodium cyanate hydrolysis re- spectively. Hydrolysis of sodium cyanate in alkaline medi- ¢>(p-1)+(2p -1) e -lio - e -plio um was also carried out under similar conditions ... (4) e= (2 ) -Ii -plio as those for urea hydrolysis (estimation of ammo- p-1 e o-pe nia). We have determined values of ¢ using Eqs (3) and (4) using computer program (FORmAN IV) Results and discussion at a given p and at different time intervals from The basic hydrolysis of urea follows a two step the value of [NH ] for a given set of reactions. reaction paths. 3 The ratios of consecutives values of () i.e., ()/ ()2' kl ()zI ()3' ()3/ ()4.... along the corresponding ratio of Urea - N!I3 + B time (//12, 12/13, Ii 14•••• ) were calculated. More- over the various trial values of p were introduced k2 B- NH3+C02 and the best value of p was selected at which the difference between the sum of squares of ratios of where B stands for cyanate. For this reaction, the () and sum of squares of ratios of time was found concentration of ammonia is related with time by to be minimum. Eq. (1). The effect of [OH-] on hydrolysis of urea was studied by carrying out a series of kinetic runs within the [OH-] range of 0.5 mol dm "? to [NH3]=Ao[2- (kl -_2~) e-k,t 3.0 mol dm - 3 at 363 K. The reaction rate was kl k2 found to be linear at low [OH-] (0.5-1.5 mol dm - 3) and a sharp increase in the reaction rate was also observed at high [OH-]. From these re- ... (1) sults it is clear that the variation of k10bs with [alkali] obeys Eq. (5). where k, and k2 are the pseudo-first order rate klobs=Bl +B2k1[OH-] ... (5) constant and Ao is the initial concentration of where B, and B2 are the empirical constants. The urea." rate constants of second step hydrolysis (kzobs) On making of substitution, was found to be independent of [alkali]. The rate constants were found insensitive to ¢=[NH liAo-2; ()= landp= k2/kl 3 «. ionic strength. Studies were carried out at differ- Eq. (1) converts to Eq. (2). ent temperatures and activation parameters, eval- uated using Arrhenius and Eyring equations with ¢(p - 1) = e - p(J - (2 p - 1) e - (J ... (2) linear least squares techniques, are given in Table 1. Equation (2) can be solved" if the value of () is The rate of the non-enzymatic degradation of guessed since the value of () and the error, e, can urea in aqueous medium was independent of pH be closely approximated from Eq. (4) between 2.0 and 12.0. The reaction rate dec- ()=()o+e ... (3) reased below pH 2.0 and increased above 1118 INDIAN j CHEM. SEC. A, DECEMBER 1996 and k20hs = k2Kh ... (7) Equation ((j) is similar to Eq.(5) with BI =k.; and These equations indicate that rate constant (k1obs) for the first step hydrolysis of urea is dependent on [OH-] and k2ob, (second step hydrolysis) is in- - ~ Q- N = C = 0 + H20'-.[ow.~N - t -0 dependent of [OH-] and confirm the observed re- sults and proposed mechanism. At low [OH-] the H2N- ~ - 0 + Hzo f~ .NH:! + co + OM 2 rate of formation of dianionic species (c) is very SchEme 2 (Slep2) slow and the reactive intermediate (b) is directly converted into the products. There, k, > k3 [OH-] and Eq. (6) reduces to pH 12.0. It has been demonstrated that at pH 7, 13 and 14 the hydrolysis of urea is an elimination reaction which gives ammonia and cyanic acid. ... (8) The fall off reaction rate below pH 2.0 is due to the protonation of urea and the dependence of The value of ko obtained from the intercept of rate on [OH-] above pH 12.0 is ascribed to base the plot of kobs versus [OH-] is 2.0 x 10 -4 min -I. catalysis of the elimination reaction. At high [OH-] (>1.5 mol dm= ') the rate of The mechanisms consistent with the observed formation of dianionic species (c) becomes quite results for both the steps of hydrolysis of urea fast in comparison to the decomposition of (b) to have been given in Schemes 1 and 2. the products. This is quite resonable to suppose The usual mechanism of alkaline hydrolysis of because the existence of a dianionic intermediate amides? that involves acyl oxygen fission by the has been observed only in strong alkaline medi- addition of hydroxide ion to the carbonyl carbon um. Therefore, k3[OH-]> k4 and ko can also be to form tetrahedral intermediate followed by its neglected at higher [OH-]. Equation (6) which re- decomposition to give products (ammonia and duces to Eq. (9) may be rearranged as Eq. (10). CO2) may be applied for urea hydrolysis. But the mechanism does not suitably explain the forma- kJ k [OH-]2 3 ... (9) tion of cyanate ion from tetrahedral intermediate.
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