Question

Thinking about a third-order reaction of the form 2A → P with kr = 6.50x10-4 dm6*mol-2*s-1,...

Thinking about a third-order reaction of the form 2A → P with kr = 6.50x10-4 dm6*mol-2*s-1, find the time required for the concentration of A to change to 0.015 mol*dm-3 from an initial concentration of 0.030 mol*dm-3.

Homework Answers

Answer #1

ANSWER:

Given,

Rate of reaction = 3rd order

kr = 6.500 x 10-4 dm6 mol-2 s-1

initial concentration, [A]o = 0.030 mol dm-3

final concentration, [A]t = 0.015 mol dm-3

For the nth order of reaction, rate law can be written as:

So, for third order (n=3) reaction, rate law is:

t = 2564076.9 sec

t = 712.24 hours

Hence, the time required for the concentration of A to change to 0.015 mol dm-3 from an initial concentration of 0.030 mol dm-3 is 2564076.9 sec (or, 712.24 hours).

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
1. Given the reaction 2A + 3B à C + 4D the reaction is zeroth order...
1. Given the reaction 2A + 3B à C + 4D the reaction is zeroth order with respect to A and second order with respect to B. If the concentration of both A and B are doubled and the temperature remains unchanged, the rate of the reaction will increase by a factor of what?   Why? 2.      The kinetics of the reaction A+B à P were studied. The following data was collected. What is the rate law for this reaction?   Why?...
The following is known about the reaction below: Chemical reaction: 2A-->2B The order of A is...
The following is known about the reaction below: Chemical reaction: 2A-->2B The order of A is second order If you start out with 2.75 M of A, after 5 minutes you will have 2.00M From these facts, determine: a) the rate law constant, K b) the first half life c) from time 0, how long will it take to reach 25% of the original concentration of A d) what is the concentration of A after 10 minutes?
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...
1.) 2A → B + C The above reaction is run and found to follow second...
1.) 2A → B + C The above reaction is run and found to follow second order kinetics with a rate constant of 1.30 x 10-3 M-1sec-1. If the initial concentration of A is 1.33 M, what is the concentration after 164 seconds? 2.) 2A → B + C Two trials of the above reaction are run with the same initial concentration of A. The first trial is performed at 25oC and the second at 35oC. If the rate constant...
Questions about biochem: 1.) If the ΔG'° of the reaction A --> B is +1000 kJ/mol,...
Questions about biochem: 1.) If the ΔG'° of the reaction A --> B is +1000 kJ/mol, under standard conditions the reaction will never reach equilibrium. True or False ? 2.) An enzyme catalyzes the reaction A↔B. The enzyme is present at a concentration of 4 nm, and the Vmax is 1.5 µM s-1. The Km for substrate A is 10 µM. Which of the following is the initial velocity of the reaction Vo when the substrate concentration is 10 µM?...
The reactant concentration in a zero-order reaction was 6.00×10−2 M after 160 s and 1.50×10−2 M...
The reactant concentration in a zero-order reaction was 6.00×10−2 M after 160 s and 1.50×10−2 M after 305 s . What is the rate constant for this reaction? (I got this answer 3.10*10^-4 M/s) What was the initial reactant concentration for the reaction described in Part A? The reactant concentration in a first-order reaction was 0.100 M after 40.0 s and 3.80×10−3M after 90.0 s . What is the rate constant for this reaction? (I got this answer 6.54*10^-2 1/s)...
If a reaction is first order with a rate constant of 5.48*10^-2 sec^-1, how long is...
If a reaction is first order with a rate constant of 5.48*10^-2 sec^-1, how long is required for 3/4 of the initial concentration of reactant to be used up?
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of...
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of the reactant is 0.0100M, what is the concentration remaining after 15 min? a) .0099M b) .0056M c) .0025M d) .0064M 2) the rate constant for the first order decomposition of A at 500 degrees Celsius is 9.2 x 10 to the negative 3rd powers s-1. How long will it take for 90.8 % of a 0.500M sample of A to decompose a) 2.5 x...
What is the half-life of a first-order reaction with a rate constant of 4.20×10−4  s−1? (the answer...
What is the half-life of a first-order reaction with a rate constant of 4.20×10−4  s−1? (the answer is 1650s) What is the rate constant of a first-order reaction that takes 458 seconds for the reactant concentration to drop to half of its initial value?
1.) The rate constant for a certain reaction is k = 3.40×10−3 s−1 . If the...
1.) The rate constant for a certain reaction is k = 3.40×10−3 s−1 . If the initial reactant concentration was 0.550 M, what will the concentration be after 20.0 minutes? 2.)A zero-order reaction has a constant rate of 1.10×10−4 M/s. If after 80.0 seconds the concentration has dropped to 9.00×10−2M, what was the initial concentration?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT