Question

The reaction A → C was performed and the concentration vs. time data below collected. time,...

The reaction

A → C

was performed and the concentration vs. time data below collected.

time, s 0 1 2 3 4 5 6 7 8
[A], mol/L 0.7905 0.5041 0.3214 0.2049 0.1307 0.08332 0.05313 0.03388 0.02160

Complete the rate law for the reaction by filling in the values for the rate constant and reaction order.

Rate = k[A]x

rate constant (without units) =

reaction order =

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
You will need to generate a set of graphs to answer this question. Concentration vs time...
You will need to generate a set of graphs to answer this question. Concentration vs time data for the following decomposition reaction was collected at 300 K. The data is shown in the table below. What is the rate constant for the reaction at this temperature (in units of min-1)? H2O2(aq) → H2O(l) + 1/2 O2(g) time (min) [H2O2](mol/L) 0 0.00915 500 0.00486 1000 0.00256 1500 0.00136 2000 0.00072
3. A certain reaction has the following general form: 2A > B Concentration vs time data...
3. A certain reaction has the following general form: 2A > B Concentration vs time data were collected for this reaction, at 50°C and an initial concentration of 0.0200 M. It is determined that a plot of ln[A] vs. time resulted in a straight line with a slope value of - 2.97 X 10-2 min-1. A. Write the rate law. B. Write the integrated rate law C. What is k for this reaction (or what is the rate constant for...
For A --> products, time and concentration data were collected and plotted as shown here. [A]...
For A --> products, time and concentration data were collected and plotted as shown here. [A] M.....t (s) .650 ..... 0.0 .575 ..... 30.0 .500 ..... 60.0 .425 ..... 90.0 Determine the reaction order, the rate constant, and the units of the rate constant. Reaction Order = ? k= ? I am having trouble figuring out the rate and reaction order. Please Help! Explain how you got the answer.
Please study the table of data below, collected for the gas phase combination reaction of N2O...
Please study the table of data below, collected for the gas phase combination reaction of N2O with O3 at 298 K and constant volume (1.00 L). Experiment [N2O]0 [O3]0 Initial rate of reaction of O3 (M/s) 1 .010 .010 6.01 x 10^-4 2 .010 .020 1.20 x 10^-3 3 .020 .020 1.19 x 10^-3 A) Please determine the order of each reactant and write the rate law for the overall reaction. B) The overall reaction is: N2O (g) + O3...
Item 4 The integrated rate laws for zero-, first-, and second-order reaction may be arranged such...
Item 4 The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line,y=mx+b. Order Integrated Rate Law Graph Slope 0 [A]t=−kt+[A]0 [A]t vs. t −k 1 ln[A]t=−kt+ln[A]0 ln[A]t vs. t −k 2 1[A]t= kt+1[A]0 1[A]t vs. t k Part A The reactant concentration in a zero-order reaction was 6.00×10−2 mol L−1 after 140 s and 3.50×10−2 mol L−1 after 400 s . What is the rate constant for...
The reaction 2NO(g)+ 2H2(g) ---> N2(g)+ 2H2O(g) was studied at 904 °C, and the data in...
The reaction 2NO(g)+ 2H2(g) ---> N2(g)+ 2H2O(g) was studied at 904 °C, and the data in the table were collected. Reaction Concentration (mol/L) Rate of Appearance of N2 [NO] [H2] (mol/L·s) 0.498 0.122 0.191 0.249 0.122 0.0478 0.249 0.244 0.0956 0.125 0.488 0.0482 A) Determine the order of the reaction for each reactant. reaction order in [NO] = ____ reaction order in [H2] = ____ B) Write the rate equation for the reaction. (Use k for the rate constant.) Rate...
The following data was collected for the reaction of ammonium ion and nitrite ion: Reaction data...
The following data was collected for the reaction of ammonium ion and nitrite ion: Reaction data for the reaction of ammonium and nitrite ions in water at 25 oC NH4+(aq) + NO2-(aq) --> N2(g) + 2H2O(l) Experiment Number Initial Concentrations (M) Initial Concentrations (M) Observed Initial Rate of Reaction (M s-1​) NH4​+ NO2- 1 0.0100 0.200 5.4 x 10-7 2 0.0200 0.200 10.8 x 10-7 3 0.0400 0.200 21.5 x 10-7 4 0.0600 0.200 32.3 x 10-7 5 0.200 0.0202...
The data below show the concentration of N2O5 versus time for the following reaction: N2O5(g)→NO3(g)+NO2(g) Time...
The data below show the concentration of N2O5 versus time for the following reaction: N2O5(g)→NO3(g)+NO2(g) Time (s) [N2O5] (mol L−1) 0 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210 Determine the order of the reaction.
TWO MOLECULES OF BUTADINEC4H6 CAN JOIN TO FORM C8H12. C4H6----1/2C8H12 THE FOLLOWING CONCENTRATION VERSUS TIME DATA...
TWO MOLECULES OF BUTADINEC4H6 CAN JOIN TO FORM C8H12. C4H6----1/2C8H12 THE FOLLOWING CONCENTRATION VERSUS TIME DATA WERE COLLECTED AT 500DEGREE C TIME(SEC) [C4H6](mol/Lu*100 TIME(SEC) [C4H6]mol/L*100) 0 ? 195 1.62 41.40 .84 604 1.47 4655 .80 1246 1.29 6210 .68 2180 1.10 8135 .57 A.DETERMINE GRAPHICALY THE ORDER OF REACTION WITH RESPECT TO C4H6,AND WRITE THE RATE LAW. B. WHAT IS THE RATE CONSTANT THE REACTION AS DETERMINED FROM THE GRAPH. C.WHAT IS THE INITIAL CONCENTRATION OF C4H6 (AT SEC) D.WHAT...
The following questions refer to the hypothetical reaction A + B → products. The kinetics data...
The following questions refer to the hypothetical reaction A + B → products. The kinetics data given can be analyzed to answer the questions. [A]0 [B]0 Rate of decrease (mol/L) (mol/L) of [A] (M/s) 5.0 5.0 X 10.0 5.0 2X 5.0 10.0 2X Time (s) [B] (mol/L) 10.0 100 20.0 100 30.0 100 Reference: Ref 12-11 The rate law for the reaction is Rate = k[A]x[B]y. What are the values of x and y?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT