Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,CI, (g) so, (g) + Cl,(g) Rate = X. + log cos. 12 Part 2 Feedback O See Hint Remember to use square brackets to show concentration. Do not include multiplication symbols in the rate equation. Do not place spaces in your answer. Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. NO,(2) +Co(e) → No(2)+Co,(e)

Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,CI, (g) so, (g) + Cl,(g) Rate = X. + log cos. 12 Part 2 Feedback O See Hint Remember to use square brackets to show concentration. Do not include multiplication symbols in the rate equation. Do not place spaces in your answer. Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. NO,(2) +Co(e) → No(2)+Co,(e)

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

Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.
Question 23 The rate law for a reaction is determined to be rate=k[AJIB}*[C]. If the reaction has an overall order of 9, what is the value of exponent for B? (the answer should be entered as a single digit number; do not enter units; examples include 0 and 1 and 2 and 3 and etc.) K Questa A Moving to another question will save this response. B88 . 43C & %23 4 5 6. 8 3 I o P Q E R T Y tab A S F G K caps lock V B alt alt control option command command option
TIA
Answer in two significant digits, please!
A chemistry graduate student is studying the rate of this reaction: NH4OH(aq)—>NH3(aq)+H2O(aq) He fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds (shown in picture). A. Write the rate law for this reaction B. Calculate the value of the rate constant k. Round your answer to two significant digits. Also be sure your answer has the correct unit symbol.
Consider the following balanced chemical equation: H₂O2 (aq) + 31 (aq) + 2 H* (aq) → 13¯ (aq) + 2 H₂O (1) In the first 49.9 seconds of the reaction, the concentration of 13 increased from 0.692 M to 0.93 M. What is the average reaction rate over this time interval (in mol L-¹ s-¹)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:
Answer all questions in this section. 1. (a) H2S(aq) + Cl2(g) – S(s) + 2HCI(aq) i. Given that, when the concentration of H2S is doubled, rate also double while double the concentration Cl2 will cause the rate of reaction increase 4 times. Write the rate law of the reaction. ii. The overall reaction order ii. The rate of reaction at 300K if the rate constant is 2.8 x 10²M²s' and the concentration of H2S and Cl2 are 2.7×10²M and 7.0x10² M respectively.
TIA
Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, fınd the rate law. 0–H [RCOOH], M [R'OH], M (HA], M Initial Rate, Ml·min' || R-c-o–H 0.35 0.35 0.50 4.60 0.50 + HA - R-Ć+ k2 0.62 0.35 8.14 A- 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 0–H Group 1 Rate = k[RCOOH][R'OH] 0–H 0–H k3 O Rate = k[RCOOH][R'OH][HA] R-C+ A + R -0–H R—С—0—Н Rate = k[RCOOR']/{[RCOOH][R'OH]} k4 0–H R'-o+ A- Rate = k[R'OH] Group 2 H Rate = k[RCOOH] 0–H k5 R—С—0—н R-C-0–R' + H2O + HA R-o+ A- Group 3 H. Step 2 or Step 3 Step 1 or Step 2 Step 1 or Step 3 Step 2 Step 1
Show your work please, thank you!
Answer the following questions from number 2 up to 5.