In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 5.00 mL 3.55 M acetone + 10.0 mL 1.80 M HCl + 10.0 mL 0.00600 M I2 + 25.0 mL H,O A student found that it took 354 seconds for the color of the I2 to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of I2 in the reaction mixture, [I2]o- Then use the equation A[12] Rate = - At t |M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H*, and iodine to I,. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). ORate Ok Om On Op O[Ace] O[H*]

In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 5.00 mL 3.55 M acetone + 10.0 mL 1.80 M HCl + 10.0 mL 0.00600 M I2 + 25.0 mL H,O A student found that it took 354 seconds for the color of the I2 to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of I2 in the reaction mixture, [I2]o- Then use the equation A[12] Rate = - At t |M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H, and iodine to I,. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H as p). c. Select all the unknown variables in the equation in part (b). ORate Ok Om On Op O[Ace] O[H*]

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

Kindly help me answer this. Will be upvoting for accurate and handwritten solutions. Thank you so much!
Show all working explaining detailly your solution. Answer Q 98, 99 & 100
Antacid Neutralization Describe the mechanism of action for each of the antacids, Be sure to indicate the base, the acid, and the product of the reaction. 中 Antacid Neutralization A. Aluminum hydroxide Al(OH)3 B. Sodium bicarbonate Al(OH),+ 3 HCI € (slow) AICls +3 H20 NaHCO, + HCI → NaCl + H20 + CO2 (fast) NaHCOз Baking soda C. Calcium carbonate CaCl; + H20 + CO2 (fast) CaCOs +2 HCI CaCO3 Generic Tums D. Magnesium hydroxide Mg(OH)2 Milk of Magnesia Mg(OH)2 + 2 HCIE MgCl; + 2 H20 (slow/moderate)
Please help explain this question... Not sure if I am doing this right. I am stuck
For items 7 - 11. Select the correct answers on each item. PS. this is not graded.
Please answer this question
O KINETICS AND EQUILIBRIUM Using a second-order integrated rate law to find concentration... -1-1 At a certain temperature the rate of this reaction is second order in Cl,0, with a rate constant of 103.Ms: 2Cl,0; (g) 2Cl, (g) +50, (g) → Suppose a vessel contains Cl,0, at a concentration of 0.130M. Calculate the concentration of Cl,0, in the vessel 0.550 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10 Check Explanation Terms of Use | Privacy Center Accessibility 2021 McGraw Hill LLC. All Rights Reserved. II
Hello i like the way u solve my question can u answer this too? Thank uuuu
Based on the result from the room temperature experiment (20°C), estimate the time it would take a piece of zinc to completely react in hydrochloric acid at a temperature of 30°C. Remember, as a general rule the rate will double for every 10°C increase in temperature. **Note: the result from the experiment was that it took Zinc 2 minutes and 27 seconds to completely react in hydrochloric acid at room temperature (20°C) a) about 1:20 b) about 0:40 c) about 5:20 d) about 13:30
5.00 mL 4.50 M acetone + 10.0 mL 1.15 M HCl + 10.0 mL 0.00200 M I2 + 25.0 mL H2O A student found that it took 146 seconds for the color of the I to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of Iz in the reaction mixture, [I2]o. Then use the equation Rate At t M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H", and iodine to I2. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). Rate O[Ace] (Previous Next
How would you find the rate law for this question?