The decomposition of urea in 0.1 M of HCl occurs according to the reaction NH,CONH, +2H,0→2NH; +CO; The first-order rate constant for this reaction was measured as a function of temperature, with the following results T /°C 61.0 Еxpt. kx 106 / min-1 1 7.13 2 71.2 27.7 Calculate the entropy of activation at 71.2 °C for the reaction of decomposition of urea. Make the assumptions you need.

The decomposition of urea in 0.1 M of HCl occurs according to the reaction NH,CONH, +2H,0→2NH; +CO; The first-order rate constant for this reaction was measured as a function of temperature, with the following results T /°C 61.0 Еxpt. kx 106 / min-1 1 7.13 2 71.2 27.7 Calculate the entropy of activation at 71.2 °C for the reaction of decomposition of urea. Make the assumptions you need.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

None
A certain reaction has an activation energy of 66.0 kJ mol' and a frequency factor of A1 = 6.80x1012 L mol 's1. What is the rate constant, k, of this reaction at 22.0 °C? Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot (asterisk) or a dash. • View Available Hint(s) HẢ X•10" k = 5.277 L•mol-1 1 •S
Consider the following mechanism in aqueous solutions. At 298 K the equilibrium constant for the first step is 5.75⋅10−35.75⋅10-3 k1k1 Step1: A + A −−→←−−←→ A + B k−1k-1 k2k2 Step2: B →→ P When [A] is large, the second step is slow and the first step is fast and at equilibrium. Under these conditions the following experimental data is gathered. The third column in the table is a check to make sure [A] is sufficiently large. The ratio should be greater than 100 when the absolute uncertainties are ±0.01±0.01 Note that as time goes on here, the assumption we are making will not work. Time…
calculate the activation energy and the frequency factor of a certain reaction, using the tabulated data below
Consider the reaction data. A⟶productsA⟶products ? (?)T (K) ? (?−1)k (s−1) 275275 0.3800.380 675675 0.7470.747 a)What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all value x1=? x2=? y1=? y2=? b)Determine the rise, run, and slope of the line formed by these points. c)What is the activation energy of this reaction?
The enzyme carbonic anhydrase catalyzes the reactionCO2(g) + H2O(l)--->HCO3- (aq) + H+(aq). In water,without the enzyme, the reaction proceeds with a rateconstant of 0.039 s-1 at 25 °C. In the presence of the enzymein water, the reaction proceeds with a rate constantof 1.0 x 106 s-1 at 25 °C. Assuming the collision factor isthe same for both situations, calculate the difference inactivation energies for the uncatalyzed versus enzymecatalyzedreaction.
Please only answer 6D
Please don't provide handwritten solution ....
The energy of activation for the reaction 2 HI - H2 + I2 is 180. kJ•mol-1 at 544 K. Calculate the rate constant using the equation k = Ae-Ea/RT, The collision diameter for HI is 3.5×10-8 cm. Assume that the pressure is 1.00 atm 4.0 M-1.s-1
Consider the reaction: NO(g) + C₂H₂(g) → HCN(g) + CO(g) + H(g), is The Arrhenius expression for the reaction is k(T) = 8.97 x 10-¹2 cm³ molec-¹ s¹ exp{-218 kJ mol-¹/RT} over the temperature range 1100 - 1500 K. Using transition state theory, calculate AH* and AS* for this reaction at 1300 K.
8. (15 marks) A reaction is written as A(g) At 298 K, k₁ =0.21 s.1. k.₁=5×10 Pa¹·s¹. B(g) + C(g). k-1 As the temperature increased from 298 K to 310 K, the values of k₁ and k., are doubled (denoted as k2 and K.2). (1) Calculate the rate constant k at 298K; (2) Calculate the activation energy of both forward and reverse reactions; (3) Calculate AH and AU for the reaction at 298K; (4) Calculate the reaction time at the whole pressure reaching to 152 kPa. The initial pressure of A(g) is 100 kPa and the reaction temperature is 298 K.
Give a reaction rate for the provided mechanism and do not include the intermediates in the final equation. 1. For the spontaneous reaction in water: Re(HzO)z + 2 KCN →Re(CN)z2 + 2K*(aq) + 2 H2O The postulate mechanism is where all species are in aqueous phase k1 Re(H₂O)2 + CN- Re(H₂O)(CN) + H₂O equilibrium Re(H₂O)(CN) + CN-I2 Re(H₂O)(CN)2-² Re(H2O)(CN)2243 Re(CN)22 + H2O k2 slow fast