Question

The decomposition of P2O5 is given by: rate = k[P2O5]. If the half-life for this reaction...

The decomposition of P2O5 is given by: rate = k[P2O5]. If the half-life for this reaction is 1400 s, about how long does it take for the P2O5 concentration to drop from 3.0 M to 0.3 M?

(1) 200 s

(2) 3000 s

(3) 4000s

(4) 4210 s

(5) 4650 s

The answer is (5) 4650s but I'm not sure how they got that. Please help, thanks!

Homework Answers

Answer #1

By seeing the rate law, we can say that it is 1st order reaction

Given:

Half life = 1400 s

use relation between rate constant and half life of 1st order reaction

k = (ln 2) / k

= 0.693/(half life)

= 0.693/(1400)

= 4.95*10^-4 s-1

we have:

[P2O5]o = 3.0 M

[P2O5] = 0.3 M

k = 4.95*10^-4 s-1

use integrated rate law for 1st order reaction

ln[P2O5] = ln[P2O5]o - k*t

ln(0.3) = ln(3) - 4.95*10^-4*t

-1.204 = 1.0986 - 4.95*10^-4*t

4.95*10^-4*t = 2.3026

t = 4650 s

Answer: option 5

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
The decomposition of hydrogen peroxide (H2O2) is a first order reaction with a rate constant 1.8×10-5...
The decomposition of hydrogen peroxide (H2O2) is a first order reaction with a rate constant 1.8×10-5 s -1 at 20°C. (a) What is the half life (in hours) for the reaction at 20°C? (b) What is the molarity of H2O2 after four half lives if the initial concentration is 0.30 M? (c) How many hours will it take for the concentration to drop to 25% of its initial value? *Help please!!!*
The decomposition of A to B is a first-order reaction with a half-life of 85.9 min...
The decomposition of A to B is a first-order reaction with a half-life of 85.9 min when the initial concentration of A is 0.483 M: A → 2B How long will it take for this initial concentration of A to decrease by 23.0%? PLEASE HURRY I DONT HAVE MUCH TIME TO ANSWER THIS
For a first-order reaction, the half-life is constant. It depends only on the rate constant k...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t1/2=0.693k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0 Part A A certain first-order reaction (A→products) has a rate constant of 4.20×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A],...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t1/2=0.693k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0 Part A A certain first-order reaction (A→products ) has a rate constant of 5.10×10−3 s−1 at 45 ∘C . How many minutes does it take for the concentration of the...
A decomposition reaction has a rate constant of 0.0037 yr −1. (a) What is the half-life...
A decomposition reaction has a rate constant of 0.0037 yr −1. (a) What is the half-life of the reaction? yr (b) How long does it take for [reactant] to reach 12.5% of its original value? yr
1.) The decomposition of phosphine (PH3) is a 1st order reaction. A.) If the half life...
1.) The decomposition of phosphine (PH3) is a 1st order reaction. A.) If the half life of the reaction is 35.0s, what is the rate constant? B.) How long will it take for 75% of the phosphine to decompose?
The half-life for the decomposition of dinitrogen pentoxide, N2O5, is independent of concentration at 298 K....
The half-life for the decomposition of dinitrogen pentoxide, N2O5, is independent of concentration at 298 K. Determine the order of reaction at this temperature, giving a justification for your answer.
the decomposition of hydrogen peroxide H2O2, is first-order reaction. the half-life of of reaction is 17.0minutes....
the decomposition of hydrogen peroxide H2O2, is first-order reaction. the half-life of of reaction is 17.0minutes. a.) What is the rate constant of the reaction? b.) If you had a bottle of H2O2, how long would it take for 80% to decompose?
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.46×10−4...
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.46×10−4 s−1 at a certain temperature. 1) What is the half-life for this reaction? 2) How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? Express your answer using two significant figures. 3) If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.80 M ? 4)...
Be sure to answer all parts. The reaction 2A → B is second order in A...
Be sure to answer all parts. The reaction 2A → B is second order in A with a rate constant of 27.9 M−1 · s−1 at 25°C. (a) Starting with [A]0 = 0.00737 M, how long will it take for the concentration of A to drop to 0.00180 M? s (b) Calculate the half-life of the reaction for [A]0 = 0.00737M. s (c) Calculate the half-life of the reaction for [A]0 = 0.00207 M. s
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT