A first order reaction is 65% complete in 280 s. How long does it take for the reaction to be 91% complete? a. 642 b. 945 c. 2752 d. 1554

a. The reactant concentration in a first-order reaction was 7.40×10−2 M after 35.0 s and 9.60×10−3 M after 75.0 s. What is the rate constant for this reaction? b. The reactant concentration in a second-order reaction was 0.460 M after 260 s and 2.40×10−2 M after 875 s. What is the rate constant for this reaction?

The first-order reaction SO2Cl2 → SO2 + Cl2 is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?   A. 104 min   B. 530 min   C. 990 min   D. 2300 min

6. What is the overall order of the following reaction, given the rate law? NO(g) + O(g) → NO2(g) + O2(g) Rate = k[NO] [O3] A. 1st order B. 2nd order C. 3rd order D. 1 order E. 0th order

18. Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. f you start with 0.051 M I2 at this temperature, how much will remain after 5.05 s assuming that the iodine atoms do not recombine to form I2? M

Section 5. For a different reaction, the plot of the natural log of concentration versus time in seconds plot was linear with a slope of -0.156 s¹. a. What is the order of this reaction? 1st order b. What is the rate law of this reaction? C. What is the integrated rate law of this reaction? d. Calculate the rate of the reaction if the concentration is 0.35 M. Show your work. Date

A particular reaction is proposed to be first order.  What plot would support this conclusion?   a. a linear plot of [reactant] versus time   b. an exponential decay of [reactant] versus time   c. a linear plot of ln [reactant] versus time   d. an exponential decay of ln [reactant] versus time

The reaction of 2N 20 5(g) 4NO 2(g) + O 2(g) is experimentally determined to be first order. What experimental data would support this conclusion? Plotting 1/ [N205] vs. time would be linear The half-life is independent of the initial concentration Doubling the initial concentration of N205 would yield a quadrupled initial rate. I. I. III. Only I. Only II. II. and III. I. and III.

At 330 degrees Celsius, the rate constant for the second order decomposition of NO2 is 0.775M ^ - 1 * s ^ - 1 the Initial concentration of NO2 is 0.0500M a. Write the rate law expression for this reaction b. What is the concentration of NO2 after 30.0 minutes? c. How long in minutes will it take the concentration to decrease to 0.0050M? d. What is the half life for this reaction? e. What effect would doubling the NO2 concentration have on the rate of the reaction?

4. The decomposition of SO₂Cl₂ is first order in SO₂Cl₂ and has a rate constant of 1.42 x 104 s-¹ at a certain temperature. a. What is the half-life for this reaction? b. How long will it take for the concentration of SO₂Cl₂ to decrease to 25% of its initial concentration? c. If the initial concentration of SO₂Cl₂ is 1.00 M, how long will it take for the concentration to decrease to 0.78 M? d. If the initial concentration of SO₂Cl₂ is 0.150 M, what is the concentration of SO₂Cl₂ after 2.00 x 10² s?