Cyclobutane decomposes to ethylene according to the equation: CH₂(g) → 2C₂H₂ (g) Determine the value of the rate constant for the reaction based on the following pressures, which were recorded when the reaction was carried out at a constant temperature in a constant-volume vessel. Round your answer to 2 significant digits. Time (s) P (mmHg) 0 2.0 x10³ 4.0 × 10³ 6.0 × 10³ 8.0 x10³ 1.0×104 Rate constant = 600. 475. 377. 299. 236. 187. -1 S x10

Cyclobutane decomposes to ethylene according to the equation: CH₂(g) → 2C₂H₂ (g) Determine the value of the rate constant for the reaction based on the following pressures, which were recorded when the reaction was carried out at a constant temperature in a constant-volume vessel. Round your answer to 2 significant digits. Time (s) P (mmHg) 0 2.0 x10³ 4.0 × 10³ 6.0 × 10³ 8.0 x10³ 1.0×104 Rate constant = 600. 475. 377. 299. 236. 187. -1 S x10

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

For the decomposition of nitrous oxide at 565 °C 2 N20(g) → 2 N2(g) + 02(g) the average rate of disappearance of N,0 over the time period from t = 0 s to t = 2.02×103 s is found to be 2.82×10 4 M/s. What is the average rate of appearance of 0, over the same time period? M/s.
Consider the reaction 5B1¯ (aq) + Br0, (aq) + 6H† (aq)→3B12 (aq) + 3H2O(1) The average rate of consumption of Br is 1.16×10-4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval? Express your answer with the appropriate units.
Consider the following rate law for the reaction A + B → products. rate = k{A}2{B}2 The reaction is order with respect to A, order with respect to B, and order overall.
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
The reaction described by H, (g) + L,(g) 2 HI(g) has an experimentally determined rate law of rate = k [H2] [I2] Some proposed mechanisms for this reaction are: Mechanism A k1 (1) H,(g) + L,(g) → 2 HI(g) (one-step reaction) Mechanism B k1 =2 I(g) k_1 (1) L(g) ; (fast, equilibrium) k2 (2) H, (g) + 2 I(g) 2 HI(g) (slow) Mechanism C k1 = 2 I(g) (fast, equilibrium) (1) k2 (2) I(g) + H, (g) HI(g) + H(g) (slow) (3) H(g) + I(g) → HI(g) (fast) Question Sourc
A reaction proceeds according to the following equation: A + 3B → 2C + 2D At an early stage of the reaction, conc. A = 1.991 M and 5.23 minutes later, conc. A= 0.861 M. What is the average rate of the reaction during this time period, expressed in units of M·s-1? Report your answer with four decimals. Enter numbers only; do not enter units.
Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2NO (g) → N₂O₂ (g) step 1 2 N₂O₂(g) + O₂ (g) Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. 2NO₂ (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. << Note: your answer should not contain the concentrations of any intermediates. rate constant 0 k₁ k₂ rate = k 1-0 010 X S
Consider the reaction 5Br−(aq)+BrO−3(aq)+6H+(aq)→3Br2(aq)+3H2O(l) The average rate of consumption of Br−is 1.75×10−4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval?