Question 6 of 8SubmitInitialTrial[A][B]Rate(M/min)10.400.200.1220.200.200.03030.400.400.2440.600.400.54A) Rate = k[A][B]B) Rate = k[A]?[B]%3DC) Rate = k[A][B]?%3DD) Rate = k[A]³[B]?E) Rate = k[A]?[B]³ Question 6 of 8SubmitWhat is the rate law for the reactionA + BC +D given the experimentaldata for four trials of initial rate?InitialTrial[A]o[B]oRate(M/min)10.400.200.120.200.200.03030.400.400.2440.600.400.54A) Rate = k[A][B]B) Rate = k[A]?[B]

Let order with respect to A is x and order with respect to B is y

Answered: Trial [A]o [B] Rate (M/min) 1 0.40 0.20…

Science

Chemistry

Trial [A]o [B] Rate (M/min) 1 0.40 0.20 0.12 2 0.20 0.20 0.030 3 0.40 0.40 0.24 4 0.60 0.40 0.54

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

Draw the starting alkene that would lead to these major products under these conditions. Drawing H₂ Pd/C 11
In a study of the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 CH 3 NC(g) CH 3 CN(g) the concentration of CH 3 NC was followed as a function of time It was found that a graph of ln[CH 3 NC] versus time in seconds gave a straight line with a slope of - 4.17 * 10 ^ - 3 * s ^ - 1 and a y intercept of -4.05 Based on this plot , the reaction is order in CH 3 NC and the rate constant for the reaction is
lanation M 0.1705 0.15 0.09571 Check 0.05 0 JUL 1011 15 Is C6H12O6 being created or destroyed by the chemical reaction? seconds If C6H12O6 is being created or destroyed, what is the rate at which it is being created or destroyed 11 seconds after the reaction starts? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. If C6H12O6 is being created or destroyed, what is the average rate at which it is being created or destroyed during the first 11 seconds of the reaction? tv 20 25.08 created O destroyed W 30 neither created nor destroyed 00 ☐ X 5 0.0 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privac
If the enzyme lactase has a Vo of 0.111111111111 mM per minute when [S] = 1.0 mM, and a Vo of 0.20 mM per minute when [S] = 5.0 mM, what is its Km? Calculate Vmax of the above enzyme (lactase). Calculate the slope on a Lineweaver-Burk plot (Km/Kmax) for the above enzyme (lactase).
Any advice
Page Grades for Nancy Duran: CHE 103 X A ALEKS - Nancy Duran - Learn × + ✰ www-awa.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IQgHlvdL2donGg9plnQUm9kiGJhghYuAiZLqZVWgwEXBsd4IBLw36AkXLcyDcVVrmllCzwt0IT1g... ? O CHEMICAL REACTIONS Limiting reactants QU N OO EXPLANATION Gaseous butane (CH₂(CH₂)₂CH3) will react with gaseous oxygen (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 2.3 g of butane is mixed with 4.49 g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 3 significant digits. The question is a limiting reactant problem. You can tell it's a limiting reactant problem by the fact that you were given the initial amounts of more than one reactant. Here is the balanced chemical equation for the reaction you will need to solve the problem: 2 CH₂ (CH₂), CH₂(g) + 130₂ (g) → 8 CO₂(g) + 10 H₂O(g) You can solve limiting reactant problems in the following three steps: Step 1: Find the initial…
Hi I need help finding the rate of disappearance and rate of appearance of NO2 for time's 200 and 300 seconds. I have pasted a screenschot of my excel data table, I just need help figuring out how to get the rate of dissapearance and appearance for NO2. Thank you so much. 1 2 3 890626695 10 11 12 13 14 15 16 17 18 19 A B C D 0 0.0062 0.0116 0.016 0.0198 0.0228 0.0256 0.0278 E F G [NO₂] Times (s) [N205] (A In[N205] 1/[N205] Rate of Di Rate of Appear 0 0.02 -3.91202 00050 100 0.0169 -4.08044 0.0142 -4.25451 200 300 400 500 H 00059 00070 0.012 -4.42285 00083 0.0101 -4.59522 00099 0.0086 -4.75599 00116 600 0.0072 -4.93367 00139 700 0.0061 -5.09947 00164 K
I need help finding the rate law for each graph. The first graph is in order zero, the middle is in order first and the last is in order second.
The following growth equation was derived for color-dyed rock candy: (R - 1.8 * 10^-3 mm/min)/(3 * 10^-3 mm/min - R) = 1/(AC^m) where R is growth rate in units [mm/min] and C is concentration of dye in parts per million (ppm). Growth rate data was collected for the following concentrations: C (ppm) 50 75 100 125 150 R (mm/min) 0.0025 0.0022 0.00204 0.00195 0.0019 What are the numerical values and units of A and m, which are both constants in the equation? For a dye concentration of 400ppm, what is the estimated growth rate? Are you confident in this estimate, why or why not?
Can you please answer the second question on the handout that is attached thank you
X2Y2 + 2Z + 2Y→ Z2 + 2Y2X Trial [X2Y2 ], (M) [Z], (M) [У, (М) Initial Rate (M/min) 1 0.25 0.11 0.33 0.025 0.11 0.33 0.2 3 0.25 0.66 0.33 0.15 4 0.25 0.11 0.66 0.025 A) What is the rate law? B) What is the rate constant? C) What is the initial rate if you have 0.061 M of X, 0.092 M of Y, and 0.043 M of Z?
[A](M) [B](M) Initial Rate (M/h) 0.244 0.247 175 Using the rate equation Rate = K[A][B]n, and the partial data table above, find k if m=1 and n=1. Please do not include units. Answer: 3,165 (2,904) 0/10 points