Question

The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus...

The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus time yields a straight line with slope 5.8×10−2 (M⋅s)−1 .

What is the value of the rate constant (k) for this reaction at this temperature?

What is the half-life when the initial concentration is 0.55 M

If the initial concentration of AB is 0.220 M , and the reaction mixture initially contains no products, what are the concentrations of A and B after 70 s ?

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
The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus...
The following reaction was monitored as a function of time: AB→A+B A plot of 1/[AB] versus time yields a straight line with slope 5.5×10−2 (M⋅s)−1 . If the initial concentration of AB is 0.250 M , and the reaction mixture initially contains no products, what are the concentrations of A and B after 80 s ?
Constants | Periodic Table The following reaction was monitored as a function of time: A→B+C A...
Constants | Periodic Table The following reaction was monitored as a function of time: A→B+C A plot of ln[A] versus time yields a straight line with slope −5.0×10−3 /s . Part A Part complete What is the value of the rate constant (k) for this reaction at this temperature? Express your answer using two significant figures. k = 5.0×10−3 s−1 Previous Answers Correct Part B Part complete Write the rate law for the reaction. Rate=k Rate=k[A] Rate=k[A]2 Rate=k[A]3 Previous Answers...
In a decomposition reaction N₂O₅ --> products, a plot of the on [N₂O₅] vs time yields...
In a decomposition reaction N₂O₅ --> products, a plot of the on [N₂O₅] vs time yields a straight line with a slope of -0.0363/s. If the initial concentration of [N₂O₅] is 4.0 M, what is the concentration after 155 seconds? What is the half-life of the reaction?
1.) For the reaction D → A + C when 1/[D] is plotted versus the time...
1.) For the reaction D → A + C when 1/[D] is plotted versus the time in seconds, a straight line is obtained whose slope is 0.054 M-1s-1. What is the concentration of D (in M) after 36.0 s if [D]o = 0.80 M? 2.) For the reaction A → B + C when [A] is plotted versus the time in minutes a straight line is obtained whose slope is -0.021 M/min. What is the concentration of A (in M)...
K II 10.) For the reaction D → A + C when 1/[D] is plotted versus...
K II 10.) For the reaction D → A + C when 1/[D] is plotted versus the time in seconds, a straight line is obtained whose slope is 0.054 M-1s-1. What is the concentration of D (in M) after 36.0 s if [D]o = 0.80 M? Hint given in feedback Hint, use the information given about the plot to determine the order of the reaction and k. Next use appropriate integrated rate equation to determine the concentration.
1. Dinitrogen pentoxide (N2O5) decomposes to NO2 and O2 at relatively low temperatures in the reaction...
1. Dinitrogen pentoxide (N2O5) decomposes to NO2 and O2 at relatively low temperatures in the reaction 2N2O5(soln) → 4NO2(soln) + O2(g) This reaction is carried out in a CCl4 solution at 45° C. The concentrations of N2O5 as a function of time are listed in the table. Plot a graph of the concentration versus t, ln (natural log) concentration versus t, and 1/concentration versus t. Graphically, determine the order of the reaction, write the rate law and calculate the value...
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...
The reaction AB(aq)→A(g)+B(g) is second order in AB and has a rate constant of 0.0122 M−1⋅s−1...
The reaction AB(aq)→A(g)+B(g) is second order in AB and has a rate constant of 0.0122 M−1⋅s−1 at 25.0 ∘C. A reaction vessel initially contains 250.0 mL of 0.180 M AB which is allowed to react to form the gaseous product. The product is collected over water at 25.0 ∘C How much time is required to produce 134.0 mL of the products at a barometric pressure of 763.7 mmHg . (The vapor pressure of water at this temperature is 23.8 mmHg.)
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each of the following different values of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. Kc= 1.8×10−2 Kc= 1.0×10−5
Consider the reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each of...
Consider the reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each of the different values of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. Kc= 1.0×10−5
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT