P17B.13 Cyclopropane isomerizes into propene when heated to 500 °C in the gas phase. The extent of conversion for various initial pressures has been followed by gas chromatography by allowing the reaction to proceed for a time with various initial pressures: PJTorr 200 200 400 400 600 600 t/s 100 200 100 200 100 200 p/Torr 186 173 373 347 559 520 where p, is the initial partial pressure and p is the final partial pressure of cyclopropane. What is the order and rate constant for the reaction under these conditions?

P17B.13 Cyclopropane isomerizes into propene when heated to 500 °C in the gas phase. The extent of conversion for various initial pressures has been followed by gas chromatography by allowing the reaction to proceed for a time with various initial pressures: PJTorr 200 200 400 400 600 600 t/s 100 200 100 200 100 200 p/Torr 186 173 373 347 559 520 where p, is the initial partial pressure and p is the final partial pressure of cyclopropane. What is the order and rate constant for the reaction under these conditions?

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

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
The gas phase decomposition of sulfuryl chloride SO₂Cl₂ → SO₂ + Cl₂ follows a first-order law. The reaction is carried out in a constant volume (V) isothermal batch reactor. For the first-order reaction, the rate r = kC₁, where C₁ (mol/liter) is the concentration of sulfuryl. And k = 3.5(e-3) min (3.1) Use the mass balance (for transient processes) to find the equation for depletion of C₁ (t) as a function of time (t). (3.2) Solve this ordinary differential equation for C₁ at t = 4 minute, using the initial condition: at t=0, C₁ (0) = 0.0284 mol/liter.
148409766/materials/gp/2496058638 (5) Practice Dashb... Desmos | Graphing... Q Learn: English voca. gy - final assessment.docx ab 2 /2 > 157% 5. Calculate AH for the reaction N2H4 (1) + O2 (g) - N2 (g) + 2 H20 (I) given the following data: 2 NH3(g) + 3 N;O(g) ----> 4 N2(g) + 3 H2O(1) AH° = -1010. kJ N2O(g) + 3 H2(g) ----> N2H¾(1) + H2O(I) AH° = -317 kJ 2 NH3(g) + 1/2 O2(g) ----> N2H4(1) + H¿O(1) AH° = -143 kJ H2(g) + 1/2 O2(g) ----> H2O(1) AH° = -286 k) ** Be sure to show all of your manipulated equations. rr Sign out
Report the reaction order from the Integrated Law method and include the best-fit trendline equation and R2 supporting your answer.