**Kinetics Question: Understanding Rate Changes**Be sure to answer all parts.By what factor does the rate shown below change if each of the following changes occurs:\[ \text{Rate} = k[ \text{BrO}_3^- ][ \text{Br}^- ] [ \text{H}^+ ]^2 \]1. **If** \([ \text{BrO}_3^- ]\) **is doubled, the rate** \[ \text{(select) by a factor of} \ \_\_ .\] 2. **If** \([ \text{Br}^- ]\) **is halved, the rate** \[ \text{(select) by a factor of} \ \_\_ .\] 3. **If** \([ \text{H}^+ ]\) **is quadrupled, the rate** \[ \text{(select) by a factor of} \ \_\_ .\]**Explanation of the Rate Law Equation Components:**- \(\text{k}\) is the rate constant.- \([ \text{BrO}_3^- ]\) represents the concentration of bromate ions.- \([ \text{Br}^- ]\) represents the concentration of bromide ions.- \([ \text{H}^+ ]^2\) represents the square of the concentration of hydrogen ions.**Analysis of Each Change:**1. Doubling \([ \text{BrO}_3^- ]\): Since \([ \text{BrO}_3^- ]\) is directly proportional to the rate, doubling this concentration will double the rate.2. Halving \([ \text{Br}^- ]\): Since \([ \text{Br}^- ]\) is directly proportional to the rate, halving this concentration will halve the rate.3. Quadrupling \([ \text{H}^+ ]\): Since the rate depends on \([ \text{H}^+ ]\) squared, quadrupling \([ \text{H}^+ ]\) will increase the rate by a factor of \(4^2 = 16\).Please ensure your answers match the proportional changes for each scenario based on the provided rate law.

Given that: Rate = k[BrO3-][Br-][H+]2 Order with respect to BrO3- = 1 Order of Br- = 1 Order of H+…

Be sure to answer all parts. By what factor does the rate shown below change if each of the following changes occurs: Rate = k[BrO; ][Br ][#*] If BrO, is doubled, the rate (select) by a factor of If Br is halved, the rate (select) by a factor of If H* | is quadrupled, the rate (select) by a factor of

Be sure to answer all parts. By what factor does the rate shown below change if each of the following changes occurs: Rate = k[BrO; ][Br ][#] If BrO, is doubled, the rate (select) by a factor of If Br is halved, the rate (select) by a factor of If H | is quadrupled, the rate (select) by a factor of

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the reaction with the rate law, Rate = k{BrO3-}{Br-}{H+}2. By what factor does the rate change if the concentration of Br- is quadrupled? Just put in the number as a whole number or fraction.
initial rate data at a certain temp is given in the table for the reaction (see image) determine the value of the rate constant assuming units of 1/s
For the rate expression below, determine the exponents x and y for the following data. Rate = k [A] [B]Y Trial [A] M 1 2 3 4 0.10 Hint 0.20 0.10 0.30 x=1, y=0 x=0, y=1 Ox=1, y=2 x= 1, y=1 x=2, y=1 [B] M 0.20 0.20 0.10 Initial rate 4.6x10-2 9.2x10-² 2.3x10-2 0.30 1.4x10-1
The reaction A+2B ——> products was found to be first order to A and second order to B. While holding the concentration of A constant , the concentration of B is increased to 3 times its initial value . By what factor does the rate of reaction increase?
A reaction has a rate law of rate= (1.25M^-2s^-1)[A][B]^2. what concentration of b would give the reaction a rate of 0.0621M/s if the concentration of a is 0.250M
Fe3+ (aq) + 7.00 SCN- (aq) → Fe(SCN)7.00 3+ (aq) 1.)Find the rate where SCN- is consumed, if Fe3+ is consumed at 1.00 M/min. 2.) Find the rate and the overall order of the rate law
For the reaction CH, OH(aq) + H* (aq) + Cl¯ (aq) → CH₂ Cl(aq) + H₂O(1) the value of [H*] was measured over a period of time. Given the data in the table, find the average rate of disappearance of H* (aq) for the time interval between each measurement. Interval: 0 s to 30.0 s reaction rate: 6.5 X10-3 reaction rate: Incorrect Interval: 30.0 s to 60.0 s 4.8 x10-3 Incorrect t (s) 0 30.0 60.0 117.0 [H+] (M) 2.34 2.12 2.00 1.83 M/s M/S Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.260 0.280 0.0119 A + B → C+ D 2 0.260 0.784 0.0933 3 0.312 0.280 0.0143 Units k = M-²s-1 M-'s-! M-s-!
- 1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0080 M's : 2 NH3 (g) → N, (g)+3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of ammonia. How much is left 2.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10 ?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0045 M's : 2 HI (g) → H, (g)+I, (g) Suppose a 250. mL flask is charged under these conditions with 350. mmol of hydrogen iodide. How much is left 80. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10
Use the provided initial rate data to derive the rate law for the reaction whose equation is: OCI (aq) + (aq) → OI¯¯(aq) + Cl¯¯(aq) Trial [OCI-] (mol/L) 1 0.0040 2 0.0020 3 0.0020 [I-] (mol/L) Initial rate (mol/L sec) 0.0020 0.00300 0.0040 0.00450 0.0020 0.00675 Determine the rate law expression and the value of the rate constant k with appropriate units for this reaction.