The overall reaction 2A + B = C + E takes place in two steps: STEP 1 (slow): A + B C + D STEP 2 (fast): D+A= E Which of the following graphs best represents how the rate of the reaction changes when the concentration [A] is increased? A T à b B U 1 A d D [A] Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. B [A] T C [A] D [A] Your answer

A chemistry graduate student is studying the rate of this reaction: CICH,CH,CI (g) → CH,CHCI (g) + HCI (g) She fills a reaction vessel with CICH,CH,Cl and measures its concentration as the reaction proceeds: [CICH,CH,CI] time (seconds) 0.0300 M 1.0 0.0208 M 2.0 0.0144 M 3.0 0.0100 M 4.0 0.00695 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Calculate the value of the rate constant k. k = 0 Round your answer to 2 significant digits. Also be ? sure your answer has the correct unit symbol.

Consider the reaction below at 100oC  T2U (g)  ⟶⟶ 2 T (g)  + U (g)  When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, which is the numerical value of the specific-rate constant, k, for this reaction?  A. 0.149 B. 0.0372 C. 0.0667 D. 0.250

Study the two-step reactions below. Reaction 1: Step 1 (slow): H,(g) + ICI(g) Step 2 (fast): HI(g) + ICI(g) HI(g) + HCI(g) I,(g) + HC(g) Reaction 2: Step 1 (fast): NO(g) + NO(g) Step 2 (slow): N,0,(g) + 0,(g) 2NO,(g) (8O'N For each two-step reaction, answer the following: a. Write the overall reaction. What substance is the reaction intermediate? b. What is the rate law for the mechanism? C. What is the molecularity of the mechanism?

A chemistry graduate student is studying the rate of this reaction: CICH,CH, CI (g) → CH,CHC1 (g)+HC1 (g) She fills a reaction vessel with CICH,CH,Cl and measures its concentration as the reaction proceeds: time [CICH,CH,CI] (seconds) 0.0200M 10. 0.0106M 20. 0.00563 M 30. 0.00299M 40. 0.00158M Use this data to answer the following questions.

One mechanism for the destruction of ozone in the upper atmosphere is Os (9) + NO(g) → NO₂(g) + O2(g) Slow NO₂(g) + 0(g) → NO(g) + O₂(g) Fast Overall reaction O3(g) + O(g) → 20₂ (g) a. Which species is a catalyst? ONO 003 002 O NO2 b. Which species is an intermediate? ONO 003 002 O NO₂ c. E₂ for the uncatalyzed reaction 03 (g) + 0(g) → 20₂ (g) is 14.0 kj. E for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 85°C? Assume the frequency factor A is the same for each reaction. Ratio = [References) Submit Answer Try Another Version frem atempt remaning (Pr Previous

A chemistry graduate student is studying the rate of this reaction: NH,ОH (аq) — NH; (аq)+ н,о (аq) She fills a reaction vessel with NH,OH and measures its concentration as the reaction proceeds: time [NH,OH] (seconds) 0.0600M 0.10 0.0385 M 0.20 0.0247M 0.30 0.0158M 0.40 0.0101 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k || x10 Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.

Kinetic data are normally presented as graphs. The following questions test your knowledge about labeling and interpreting graphs correctly. [B] is used to represent the concentration of a reactant B in a reaction. y y LLLE 44 X X B с Decide if each of the following statements is True or False. y A y Consider graph D: if y = 1/[B] and x = time, the graph could represent a first order reaction. Consider graph A: if y = [B] and x = time, the graph could represent a first order reaction. ✓Consider graph C: if y = In[B] and x = time, the graph could represent a second order reaction. ✓Consider graph C: if y = [B] and x = time, the graph could represent a zero order reaction. ✓Consider graph D: if y = 1/[B] and = time, the slope is equal to -k. ✓ Consider graph B: if y = [B] and x = time, the graph could represent a second order reaction. X D

A chemistry graduate student is studying the rate of this reaction: 2HI (g) → H₂ (g) +1₂ (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 0.0400M 0.0199M 0.20 0.0133 M 0.30 0.00994M 0.40 0.00795 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 X Ś

What is the average reaction rate for 2 NOB1(g) → Br,(g)+2 NO(g) over the first 10 seconds? Time [NOBr] (s) (mol/L) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 [NOBI] (mol/L) mol/L 0.0100 0.0090 0.0080 0.0070 0.0060 0.0050 0.0040 0.0030 0.0020 0.00 5.00 10.00 time (s) 6.7 x 10-3 M/s d. 3.4 x 10-4 Mls a. b. 6.7 x 10-4 Mls e. 1.3 x 10-3 M/s c. 3.3 x 10-3 M/s Oxygen gas is formed by the decomposition of potassium chlorate at high temperatures according to the reaction 2 KC10, (s) → 2 KCI(s)+3 O,(g). Suppose 1.23 g KCIO; is placed in a container connected to an open-end mercury manometer on a day when atmospheric pressure is 1.00 atm. Once the reaction is complete, the height of the mercury column in the U-tube on the side of the reaction container rises by 172 mmHg. What is the pressure of O2 gas produced by the reaction? d. 0.774 atm e. 36.7 in Hg a. 1348 torr b. 22.9 kPa c. 0.559 bar