Question

At a certain temperature the rate of this reaction is first order in HI with a...

At a certain temperature the rate of this reaction is first order in HI with a rate constant of :0.0632s

2HIg=H2g+I2g Suppose a vessel contains HI at a concentration of 1.28M . Calculate how long it takes for the concentration of HI to decrease to 17.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the first-order reaction described by the equation cyclopropane---propene At a certain temperature, the rate constant...
Consider the first-order reaction described by the equation cyclopropane---propene At a certain temperature, the rate constant for this reaction is 5.42× 10–4 s–1. Calculate the half-life of cyclopropane at this temperature. Given an initial cyclopropane concentration of 0.00510 M, calculate the concentration of cyclopropane that remains after 1.70 hours.
A certain reaction is first order in H2 and first order in I2. Use this information...
A certain reaction is first order in H2 and first order in I2. Use this information to complete the table below. Round each of your answers to 3 significant digits.. [H2] [I2] Initial Rate of Reaction 0.949M. 1.59M. 3.00 X 10^3 M/s 0.949. 0.694 ? 2.03 0.742 ?
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)...
The following reaction is first order in N2O5 : N2O5 (g)→ NO3(g) + NO2(g) The rate...
The following reaction is first order in N2O5 : N2O5 (g)→ NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s Calculate the rate of reaction when [N2O5]=0.055M What would the rate of reaction be at the same concentration if the reaction was second order? Zero order? (Assume same numerical value for the rate constant but with correct units)
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4...
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4 s−1 at a certain temperature. If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.72 M ? If the initial concentration of SO2Cl2 is 0.175 M , what is the concentration of SO2Cl2 after 460 s?
At a certain temperature, the half-life of the first order decomposition of iso-propanol (shown below) is...
At a certain temperature, the half-life of the first order decomposition of iso-propanol (shown below) is 4.30 hr. iso-propanol   → propanone + dihydrogen Answer the following questions about the decomposition of iso-propanol and report all answers to three significant figures. 1. If the initial concentration of iso-propanol is 5.16×10-3 M, calculate the time (in hr) required for the concentration of iso-propanol to decrease to 57.8 % of the initial concentration. 2. If the initial concentration of iso-propanol is 5.16×10-3 M,...
Part A : A certain first-order reaction (A→products) has a rate constant of 9.30×10−3 s−1 at...
Part A : A certain first-order reaction (A→products) has a rate constant of 9.30×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? Part B : A certain second-order reaction (B→products) has a rate constant of 1.10×10−3M−1⋅s−1 at 27 ∘C and an initial half-life of 278 s . What is the concentration of the reactant B after one half-life?
a) At a certain temperature, the rate constant for this reaction is 5.09× 10–4 s–1. Calculate...
a) At a certain temperature, the rate constant for this reaction is 5.09× 10–4 s–1. Calculate the half-life of cyclopropane at this temperature. b) Given an initial cyclopropane concentration of 0.00190 M, calculate the concentration of cyclopropane that remains after 2.40 hours.
Part A A certain first-order reaction (A→products) has a rate constant of 7.20×10−3 s−1 at 45...
Part A A certain first-order reaction (A→products) has a rate constant of 7.20×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? Express your answer with the appropriate units. Answer: 6.42 min Part B A certain second-order reaction (B→products) has a rate constant of 1.35×10−3M−1⋅s−1 at 27 ∘Cand an initial half-life of 236 s . What is the concentration of the reactant B after...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A]=[A]0e−kt Now say we are particularly interested in the time it would take for the concentration to become one-half of its inital value. Then we could substitute [A]02 for [A] and rearrange the equation to: t1/2=0.693k This equation caculates the time...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT