In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH4NCO(aq)(NH2)½CO(aq) the following data were obtained: NH,NCO], M 0.715 8.95x10-2 1.05x103 0.358 0.179 minutes 150 449 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.715 M is | min and when the starting concentration is 0.358 M is min. (2) The average A(1/[NH,NCO]) / At from t = 0 min to t = 150 min i [ The average A(1/[NH4NCO]) / At from t= 150 min to t = 449 min is | M' min. м' min'. (3) Based on these data, the rate constant for this | order reaction is м' min'.

In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH4NCO(aq)(NH2)½CO(aq) the following data were obtained: NH,NCO], M 0.715 8.95x10-2 1.05x103 0.358 0.179 minutes 150 449 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.715 M is | min and when the starting concentration is 0.358 M is min. (2) The average A(1/[NH,NCO]) / At from t = 0 min to t = 150 min i [ The average A(1/[NH4NCO]) / At from t= 150 min to t = 449 min is | M' min. м' min'. (3) Based on these data, the rate constant for this | order reaction is м' min'.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter21: Rates Of Chemical Reactions, Ii. A Clock Reaction

Section: Chapter Questions

Problem 2ASA

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In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH,),CO(aq) the following data were obtained: (NH,NCO], M 0.146 1.83x10 2 S.66x10 7.30x102 3.65x102 minutes 2.44x10 812 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.146 M is concentration is 7.30x102 M is min and when the starting min. (2) The average A(1/[NH,NCO]) / At from t= 0 min to t- 812 min is The average A(1/[NH,NCO]) / At from t= 812 min to t= 2.44x103 min is M1 min M' min . (3) Based on these data, the rate constant for this v order reaction is M1 min !
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3-1/2 N2 + 3/2 H, the following data were obtained: NH3), M 3.90x10-3 1000 1.95x10-3 1.50x103 9.75x10-4 1.75x103 7.80x10-3 seconds Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 7.80×10-3 M is| s and when the starting concentration is 3.90x103 M is (2) The average rate of disappearance of NH3 from t= 0 s to t= 1000 s is Ms!. (3) The average rate of disappearance of NH3 from t = 1000 s to t= 1.50×103 s is ]Ms!. (4) Based on these data, the rate constant for this Ms!. order reaction is
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3-1/2 N₂ + 3/2 H₂ the following data were obtained: [NH3], M seconds 5.79x10-3 0 2.90x10-3 998 1.45x10-3 7.25x10-4 1.50x10³ 1.75x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 5.79x10-³ M is starting concentration is 2.90x10-³ M is S. (2) The average rate of disappearance of NH3 from t = 0 s to t = 998 s is (4) Based on these data, the rate constant for this (3) The average rate of disappearance of NH3 from t = 998 s to t = 1.50x10³ s is order reaction is M s ¹. M S-1 Ms¹. s and when the
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3 →1/2 N2 + 3/2 H, the following data were obtained: 2.00×103 5.00x104 1.50x103 1.00x10-3 2.50x104 1.75x103 NH3), M seconds 998 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.00x10 3 M is s and when the starting concentration is 1.00x10 M is (2) The average rate of disappearance of NH3 from t =0s to t = 998 s is |Ms. (3) The average rate of disappearance of NH3 from t= 998 s to t=1.50x103 s is |Ms.
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3-1/2 N2 + 3/2 H, the following data were obtained: NH3), M seconds 2.46x10-3 1.23x10-3 999 6.15x104 1.50x103 3.08x10-4 1.75x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 2.46×103 M is Mis s and when the starting concentration is 1.23x10-3 (2) The average rate of disappearance of NH3 from t = 0 s to t= 999 s is Ms!. (3) The average rate of disappearance of NH3 from t= 999 s to t= 1.50×103 s is |Ms!. (4) Based on these data, the rate constant for this v order reaction is Ms!
In a study of the decomposition of ammonia on a platinum surface at 856 °C NH3¬1/2 N2 + 3/2 H, the following data were obtained: NH3), M 1.95x10-3 1.50x103 9.75x10-4 1.75x103 7.80×10-3 3.90x10-3 seconds 0 1000 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 7.80×103M is s and when the starting concentration is 3.90×103 Mis (2) The average rate of disappearance of NH3 from t= 0 s to t= 1000 s is ]Ms!. (3) The average rate of disappearance of NH3 from t= 1000 s to t= 1.50×103 s is ]Ms!. (4) Based on these data, the rate constant for this v order reaction is Ms!
To study the photochemical decomposition of aqueous bromine exposed to bright sunlight, we dissolved a small amount of liquid bromine in water contained in a glass jar and placed under direct sunlight. The following data were obtained at 25\deg C:\table [[Tiempo (min ), 10, 20, 30, 40, 50, 60], [Ppm, 2.45, 1.74, 1.23, 0.88, 0.62, 0.44]] Determine the reaction rate order and the specific reaction rate constant: a) Differential method ( The method for obtaining the derivatives is left to your decision) Tiempo (min) Ppm Br₂ 10 2.45 20 1.74 Ć 30 1.23 40 0.88 50 0.62 60 0.44
In a study of the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °CCH3NC(g)CH3CN(g)the concentration of CH3NC was followed as a function of time.It was found that a graph of ln[CH3NC] versus time in seconds gave a straight line with a slope of -4.38×10-3 s-1 and a y-intercept of -2.83 . Based on this plot, the reaction is ______ order in CH3NC and the half life for the reaction is _______ seconds.
3. (а) A laboratory manager performed an experiment to investigate the hydrolysis of 2-chlorooctane at different temperatures. The following results were obtained: Temperature (°C) Rate constant, k, (s1) | 1.06 x 10-5 | 3.19 x 10-4 | 9.86 x 104 | 2.92 x 10-3 25 35 45 Using a graphical method, calculate pre-exponential factor k value at 50 °C (ii) (ii)
write the mechanism 2.3 NaOH, H₂O & Heat
An enzymatic hydrolysis of fructose-1-phosphate, fructose-1-P + H20 fructose + Pi was allowed to proceed to equilibrium at 25°C. The concentrations used in the reaction were lower than typical because a delicate enzyme was used - this is a typical modification used by biochemists that are valid for biochemical standard state (in this context). The original concentration of fructose-1-P was 0.2M, but when the system had reached equilibrium the concentration of fructose-1-P was only 6.52 x 10 5 Which of the below values comes closest to representing the free energy of hydrolysis of fructose-1-P?
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