It was discovered that the rate law for this reaction is given by the following equation: d[CS2] (3. 1. .07 x 10-4 dt a. How much time, in seconds, will it take for the CS2 concentration to fall from its initial concentration of 0.0500 mol/L to half of that value? b. How much time, in seconds, will it take for the CS2 concentration to fall from its initial concentration of 0.00500 mol/L to half of that value?

It was discovered that the rate law for this reaction is given by the following equation: d[CS2] (3. 1. .07 x 10-4 dt a. How much time, in seconds, will it take for the CS2 concentration to fall from its initial concentration of 0.0500 mol/L to half of that value? b. How much time, in seconds, will it take for the CS2 concentration to fall from its initial concentration of 0.00500 mol/L to half of that value?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.3: Rate Law And Order Of Reactions

Problem 11.4PSP

See similar textbooks

Similar questions

For a first-order reaction, it takes just 101 s until exactly 10.0% of the reactant is consumed. Using the equation at the bottom of page 2.4 of the Lab Manual, calculate the rate constant, k. Note: Check your significant figures! 2. The general expression for determining the rate of a first-order reaction: Reaction: A --> B Expression: Rate = k[A] Using this expression, determine the Rate when: k = 0.00035 s-1 [A] = 0.05273 mol L-1 Note: Round your answer to 3 significant figures. Please type answer not write by hend
A--> B + C is 1st order. If rate = 2 x 10^-4 when [A] = 0.1 M what is the rate when [A] = 0.5 M?
2H2O2(aq) --> 2H2O(l) + O2(g) rate expression: rate = k[H2O2]m[I-]n 1. a) What experimental factors change the numerical value of n in the rate law for the reaction of H2O2 with I-? b) What experimental factors change the numerical value of k in the rate law for the reaction of H2O2 with I-?
An experiment was conducted to determine the over-all order of the reaction:YOI ➔ MIYA At the start of the reaction, the concentration of YOI is equal to 5.142 M. After 118.0 seconds, its concentration was reduced to 2.361 M. Meanwhile, another run of the same reaction but with 3.789 M [YOI]0 showed that after 110.0 seconds, a 1.350 M decrease in concentration of YOI was observed. Based on these:1. Estimate the order of the reaction. (Answer: 2nd order)2. How much YOI will be consumed if a run with [YOI]0 = 1.234 M is allowed to form MIYA for 4.00 minutes. (Answer: 0.320M) SHOW THE COMPLETE SOLUTION. THE ANSWER SHOULD BE THE ONES INDICATED ABOVE.
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.360 0.330 0.0164 2 0.360 0.660 0.0164 3 0.720 0.330 0.0656 ?=? Units =?
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in chromium(III) ion, Cr3+ Cr3+(aq) + SCN(aq) → Cr(SCN)2+(aq) The rate constant for the reaction is (3.10x10^0)x10-6/s. What is the half-life, in seconds, for the reaction? Express yoyr answer to three significant figures.
The reaction of nitrogen dioxide with carbon monoxideNO2 + CONO + CO2is second order in NO2 and zero order in CO.Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 0.577 Ms-1 when [NO2] = 0.852 M and [CO] = 0.321M. From this experiment, the rate constant i
Part A Consider the reaction 2H3PO4→P2O5+3H2O2H3PO4→P2O5+3H2O Using the information in the following table, calculate the average rate of formation of P2O5P2O5 between 10.0 and 40.0 ss. Time (ss) 0 10.0 20.0 30.0 40.0 50.0 [P2O5][P2O5] (MM) 0 2.50×10−3 5.50×10−3 7.30×10−3 8.50×10−3 9.10×10−3
I need help step step on how tpo calculate (In). I have no idea how to get this number. The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq) H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of .00110 min-1. If the initial concentration of H2O2 is .0302M, the concentration of H2O2 will be __________M after 1144.0 min have passed.
The reaction, A → products, is known to be first order with respect to the concentration of A and first order overall. The rate constant for the reaction is 0.0400 min-1 at a certain temperature.If the initial concentration of A is 1.600 M. What will be the concentration of A after 22.5 min?Answer M How long would it take for 40.0% of the starting material (A) to undergo reaction?Answer min
The following questions refer to the gas-phase decomposition of ethylene chloride. C2H5Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction: Time (s) ln [C2H5Cl] (M) 1.0 –1.625 2.0 –1.735 What is the rate constant for this decomposition? *Side note: The answer to this problem is 0.11/s but I am unsure how to get there.*
Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+DA+2B⟶C+D Trial [?] (?)[A] (M) [?] (?)[B] (M) Rate (M/s) 1 0.2100.210 0.3000.300 0.02210.0221 2 0.2100.210 0.6000.600 0.02210.0221 3 0.4200.420 0.3000.300 0.08840.0884