What is the rate law for the reaction 2A+2B + 2C → products Initial [A] Initial [B] Initial [C] rate 0.273 0.763 0.400 3.0 0.819 0.763 0.400 9.0 0.273 1.526 0.400 12.0 0.273 0.763 0.800 6.0 rate = k[A][B][C] b. rate = k[A][B]°[C] c. rate = k[A]°[B]*[c]? d. а. с. rate = k[A]°[B]°[C] %3D

What is the rate law for the reaction 2A+2B + 2C → products Initial [A] Initial [B] Initial [C] rate 0.273 0.763 0.400 3.0 0.819 0.763 0.400 9.0 0.273 1.526 0.400 12.0 0.273 0.763 0.800 6.0 rate = k[A][B][C] b. rate = k[A][B]°[C] c. rate = k[A]°[B]*[c]? d. а. с. rate = k[A]°[B]°[C] %3D

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

Related questions

Q: What is the value of the specific rate constant, k, for this reaction: CO (g) + NO2 (g)…

Q: The tabulated data were collected for this reaction: CH3CI(g) + 3 Cl2(g) → CCI4(g) + 3 HC1(g)…

A: The kinetics data for the reaction given is,

Q: Initial‑rate data at a certain temperature is given in the table for the reaction…

A: Given,The reaction:N2O3 (g)→ NO(g) + NO2(g)[N2O3] Initial rate ( M/s)0.100…

Q: < JAL (M) 0.150 0.450 0.450 [B], (M) 0.300 0.300 0.150 Question 5 of 5 Using the information in the…

Q: e rate law

Q: For the reaction 3AE) + 2B(g) - 2C(g) + 2D(g) the following data were collected at constant…

Q: [A] vs Time In[A] vs Time O 1/[A] vs Time O Least Squares Plot Time, s The reaction A - C was…

A: Reaction = A → C For the given concentration vs time data above, we plot the…

Q: A scientist evaluated reaction rates for the reaction A + B --> C using differing initial…

Q: Consider the following data for the reaction: A+B → C+D [A] (M) [B] (M) 0.0100 0.0200 0.0200 0.0100…

Q: 6. For the reaction 2A(g) + B(g) + 2C(g) → D(g) + E(g) the following data were collected at constant…

Q: Calculate the value of the rate constant

Q: Consider this data associated with the reaction: A + B → Product The data comes from 3 experiments…

Q: Consider the following reaction. Calculate the rate of reaction for trial 4.. 2 A + B →→ 3 C…

Q: Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2…

A: A question based on kinetics of reactions in solution that is to be accomplished.

Q: e rate constant

Q: Given the info below, determine the rate law for the reaction and the rate constant (k). Be sure to…

Q: 4. The initial rate of the reaction: BrO4 (aq)+ 5 Br +8 H has been measured at the reactant…

A: Given,The reaction:

Q: A kinetics study had these data for the reaction A +B+C Products. JA]o (M) Blo (M) Initial Rate…

A: Recall the given reaction A + B + C→ProductsLet order of this reaction with respect to A is…

Q: For the reaction 2 A + B + C, the initial rate is measured at several different reactant…

A: The rate law of the reaction has to be given,

Q: oncentrations of A. A](M) Initial Rate (M/s) D.15 6.87x10-3 D.30 2.75x10-2 D.60 1.10x10 1 What is…

A: The question is based on the concept of chemical kinetics. It involves determination of rate law…

Q: What is the rate law for the reaction A + 3B products Initial [A] Initial [B] rate 0.2 0.7 3.0…

Q: Concentration and rate data are provided in the table below for the reaction shown. 2NO(g) + Cl,(g)…

A: First find the orders with respect to NO and Cl2 then find k . Put these values in data 4 to find…

Q: Consider the data table below for the generic reaction A + B → products Trial [A] (M) [B] (M)…

A: The given reaction is: A + B → products The rate law for the above reaction can be written as:…

Q: The generic rate law equation is: rate = k[A]x[B]y What is the value of y?

Q: A scientist evaluated reaction rates for the reaction A + B --> C using differing initial…

A: Chemical Reaction => A + B --> C Collected Data => [A] (M) [B] (M) Rate…

Q: NO2 + 03 NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 × 10-3 1.89 x 10-2 3.15 x 10-3 Experiment 1 0.21…

A: First, rate law is written to solve the question Rate= k[NO2]x[O3]y..............equation 1 where k…

Q: Consider the following reaction. Calculate the value of the rate constant.. 2 A + B → 2 C…

Q: For the reaction N2O5(g) → N20(g) + 202(g), the following three plots were made. What is the…

A: By seeing the plot give we can Apply the equation and find out the order of the reaction.

Q: Expt [NO2]t=0 [CO]t=0 initial rate (M/s) 1 0.10 0.10 0.0050 2, 0.40 0.10 0.080 3) 0.10 0.20 0.0050…

A: Chemical kinetics is the study of the reaction that how fast or slow a reaction is taking place. The…

Q: Consider the following reaction data. Reaction [A] (M) [B] (M) Rate (M/s) 1 0.100 0.100 10 2 0.200…

Q: initial rate Consider the following reaction and initial rate data: Experiment 1 2 3 4 2H₂(g) + 2NO…

Q: Select the rate law that corresponds to the data shown for the following reaction: A+B → C EXP 1 2 3…

A: d) rate=k[B]3Explanation:Step 1:Step 2:Step 3:

Q: M

A: Dear student I have given answer to your question in the image format.

Q: Given the information below, determine the rate law for the reaction and the rate constant (k). Be…

A: Rate law: K[A]2[B]1 Rate constant K = 1.5 M-2s-1

Q: ConsideT the tablE ol data collected for the reaction A → Products. Determine the magnitude (value)…

A: Given that Reaction A ---------> product

Q: 12 2.00 x 10-2 (a) What is the average rate of reaction between 1 and 4 h? Report the units as well…

A: The given first order reaction is :A → B + CThe data showing change in concentration of A with…

Q: Consider the following reaction. Calculate the value of the rate constant.. 3 A + B → 2 C…

A: The reaction 3 A + B → 2 CTrial [A]0[B]0[C]0Rate (M/s)10.610.150.071 3.01321.220.150.07112.052…

Q: Consider the initial-rate data at a certain temperature in the table for the reaction described by 2…

Q: scientist evaluated reaction rates for the reaction A + B --> C using differing initial…

A: The given reaction is : A + B --> C Let the rate law for the reaction: Rate =k [A]x[B]y Here x…

Q: Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [02], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21…

A: Reaction :- NO2 + O3 ---> NO3 + O2 Reaction is balanced Rate = (1/coefficient)…

Q: The following initial rate data were obtained Initial [NO₂] Initial [CO] Initial Rate Experiment…

Q: NO2(e) + CO(g) NO(g) + CO2(g) Rate (M/sec) Initial [NO2] Initial [CO ] 1.1 x 10-2 0.15 0.1 4.5 x…

Question

What is the rate law for the reaction 2A + 2B+ 2C → products
Initial [A]
Initial [B]
Initial [C]
rate
0.273
0.763
0.400
3.0
0.819
0.763
0.400
9.0
0.273
1.526
0.400
12.0
0.273
0.763
0.800
6.0
rate = k[A][B][CỊ
b. rate = k[A][B]'[C]
c. rate = k[A]°[B]*[C]?
d. rate = k[A]°[B]°[C]?
а.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Consider the reaction: A -----------> 2C The concentration of reactant A and product B were monitored at the same time interval. Time t, Minutes Molar Concentration A, [A] Molar Concentration C, [C] 0 2.40 0.00 2.00 2.20 0.40 4.00 2.00 0.80 Identify the correct rate of the reaction. 0.00 0.40 0.80
Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO₂(g) + O₂(g) → N₂O5 (g) + O₂(g) Determine the value and units of the rate constant, k. k = X10 TOOLS [NO2], (M) [03]o (M) 0.650 0.800 1.10 0.800 1.76 1.40 Units: Initial rate (M/s) 3.12 x 104 5.28 x 104 14.78 x 104
For the reaction A → products, concentration and time data were collected. Enter these data into the graphing tool to determine the reaction order. t Graphing Tool 0.0 25.0 50.0 73.0 [A] 3.40 2.28 1.53 1.02 In[A] 1.223775 0.824175 0.425268 0.019803 Clear All Data 1/[A] 0.294118 0.438596 0.653595 0.980392 [A] 3.4 2.822 2.244 1.666 1.088 0.51 [A] vs. t to 0 14.6 t (s) 0.0 25.0 50.0 75.0 In[A] vs. t 29.2 t 43.8 1/[A] vs. t 58.4 [A] (M) 3.40 2.28 1.53 1.02 73
In a reaction where A and B go to products, what is the rate law if the following rates are observed? [A] mol/L [B] mol/L rate M/s 0.020 0.010 0.278 0.040 0.010 0.556 0.030 0.020 1.67 0.040 0.020 2.22 rate = k[A][B]? B rate = k[A]°[B] rate = k[AJ°[B]? rate = k[A][B]
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
X2 + Y₂ → 2Z R = k[Y₂] Trial [X₂]. (M) [Y₂], (M) Initial Rate (M/hr) 1 0.100 0.100 2.15 x 10-3 2 0.100 0.300 6.45 x 10-3 3 0.300 0.200 4.30 x 10-³ What is the rate constant for the reaction given the rate law and data? k = [?] Enter the answer choice number. Rate Law Expression Enter
Consider the reaction I- + OCl- → OH-→ IO- + Cl- Determine the reaction's rate law using the given experimental data. Exp # [I-]o [OCl-]o [OH-]o Initial Rate (M/s) 1 0.0013 0.012 0.10 0.094 2 0.0026 0.012 0.10 0.187 3 0.0013 0.006 0.10 0.047 4 0.0013 0.012 0.20 0.047
6
9.
Consider the data shown here for the reaction NO2(g) + CO(g) -> NO(g) + CO2(g) The data shows the initial rate for the reaction for various concentrations of reagents. Expt L[NO2]t=0 [CO]t=0 initial rate (M/S) 0.0050 0.10 0.40 0.10 0.10 0.080 0.10 0.20 0.0050 What is the order of this reaction with respect to CO ? Oa. 2 Ob. 1 Oc. o 123
What is the rate of the reaction when A=0.43M and B=0.31M?
Consider the reaction between nitric oxide and hydrogen 2NO + H2 → N20 + H20 Initial Rate of Disappearance of NO Experiment Initial [NO], M Initial [H2], M (mol/L sec) 1 6.4 x 10-3 2.2 x 10-3 2.0 x 10-5 2 12.8 x 10-3 2.2 x 10-3 8.0 x 10-5 6.4 x 10-3 4.4 x 10-3 4.0 x 10-5 What is the rate law for this reaction? a. Rate = k[NO] b. Rate = k[NO]? c. Rate = k[NO]²[H2] d. Rate = k[No][H2]