Chemistry

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26 Nov 2019

Imagine that you took a road trip. Based on the information in the table, what was the average speed of your car?

Time Mile marker

3:00 pm 13

8:00 pm 300

Now consider the following reaction and data:

H2+2IBrâ2HBr+I2

Time
(s) I2 concentration
(M)

5 1.22

15 1.73

What is the average rate of formation of I2?

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Reid WolffLv2

15 Aug 2019

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BASED ON PART B, PLEASE ANSWER C AND D WITH CORRECT UNITS. THANKS!

Part A

Imagine that you took a road trip. Based on the information in the table, what was the average speed of your car?

Time	Mile marker
3:00 pm	31
8:00 pm	208

Express your answer to three significant figures and include the appropriate units. Use mi as an abbreviation for miles, and h for hours, or mph can be used to indicate miles per hour.

= 35.4 mph

Now consider the following reaction and data:

H2+2BrClâ2HCl+Br2

Time (s)	Br2concentration (M)
5	1.30
15	1.95

Part B

What is the average rate of formation of Br2?

Express your answer to three decimal places and include the appropriate units.

= 0.065 Ms

Part C

Based on your answer to Part B, what is the average rate of formation of HCl?

Express your answer to three decimal places and include the appropriate units.

Part D

Based on your answer to Part B or C, what is the average rate of change of H2? Remember that reactant concentrations decrease over time.

Express your answer to three decimal places and include the appropriate units.

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The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

Show transcribed image text The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

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