The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 x 10 s' at 593 K What percentage of the initial amount of SO2C12 will remain after 9.2 hours? O 100% 99.9% 3.88% 48.3% 2.20%

The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 x 10 s' at 593 K What percentage of the initial amount of SO2C12 will remain after 9.2 hours? O 100% 99.9% 3.88% 48.3% 2.20%

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

-1. Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0058 M-s: 2N₂O(g) → 2N₂ (g) +0₂ (8) Suppose a 2.0 L flask is charged under these conditions with 450. mmol of dinitrogen monoxide. After how much time is there only 225. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 S Ala X 2. ?
What percentage of the initial amount of S02Cl2 2ilk remain after 2.25 hours?
A particular reactant decomposes with a half-life of 173 s when its initial concentration is 0.301 M. The same reactant decomposes with a half-life of 231 s when its initial concentration is 0.225 M. Determine the reaction order. 01 0 2 What is the value and units of the rate constant for this reaction? k = Units
Consider the gas-phase reaction: H2(g) + 12(g) → 2 HI(g) The reaction was experimentally determined to be first order in H₂ and first order in 12. Consider the proposed mechanisms. Mechanism 1: H2(g) + 2(g) 2 HI(g) single step k₁ Mechanism 2: 12(g) k_1 21(g) fast H2 212 HI(g) slow K2 *Draw energy diagrams for the mechanisms shown: Show that both of the proposed mechanisms are valid.
KINETICS AND EQUILIBRIUM Identifying intermediates in a reaction mechanism Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. ☐ yes no (1) (2) ローロ 00 09 0.0.... X Ś 0/3
Using the data in the table, calculate the rate constant of this reaction. k= A+B → C + D Trial [A] (M) [B] (M) 1 0.290 0.380 2 0.290 1.03 3 0.464 0.380 Units Rate (M/s) 0.0163 0.119 0.0261
Consider the reaction below and the proposed mechanism. X2 + Y + Z → XY + XZ Step l) X2 + Y → XY + X (very slow) Step 2) X + Z → XZ (very fast) What is the rate law for this reaction if the proposed mechanism is correct?
The isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the equations above. Here C3H6* is an excited cyclopropane molecule. At low pressure, Step 1 is much slower than Step 2. Derive the rate law for this mechanism at low pressure?
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
The gas phase decomposition of sulfuryl chloride at 600 K SO₂ Cl₂ (g) → SO₂ (g)+ Cl₂ (g) is first order in SO₂ Cl2 with a rate constant of 2.80 × 10-³ min-¹. If the initial concentration of SO₂ Cl2 is 0.00164 M, the concentration of SO₂ Cl2 will be 0.000364 M after min have passed.
At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś