Share
Explore BrainMass

Explore BrainMass

  1. Chemistry
  2. Physical Chemistry
  3. Chemical Kinetics
  4. 1635

Determining the Order of a Chemical Reaction

In an aqueous solution, glucose decomposed according to the results shown below.
(a) Demonstrate that the reaction is first order.
(b) Calculate the rate constant for the decomposition process.
(c) Calculate the half-life (t1/2) for glucose under the specified conditions.

Glucose decomposition results:
Time (min), Glucose conc. (mM)
0, 28.0
22.5, 27.7
60, 27.1
120, 26.3
240, 24.5

Solution Preview

The attached file contains a complete solution.

To show that the reaction is first order, plot the experimental data according to the equation for a first order reaction:

ln[G]=ln[G]o-kt, where
[G] = concentration of glucose
[G]o = concentration of glucose at time zero
k = rate constant
t = time

The above equation is in the form of a linear relation (y=slope*x+intercept), where y=ln[G], ...

$2.19

Related Solutions

Second Order Reaction

For the second order reaction below, the initial concentration of A is 1.34M. If k=7.61x10(exponent negative 4) seconds(exponent negative 1), what is the concentration of A after 18.3 minutes? 2A-->B rate=k[A](exponent2)

Rate law of chemical reaction

The rate of the following reaction in aqueous solution is monitored by measuring the rate of formation of (I3^-). The data obtained is listed in the table. (S2O8^2-) + (3I^-) ----> (2SO4^2-) + (I3^-) Experiment ([S2O8]^2-), M ([I]^-),M Initial rate, M s^1- 1 0

Chemical Kinetics, Experimental Measurements and Rate Law

1) Explain the concept of chemical kinetics and the various factors that influence reaction states. 2) Relate experimental measurements to reaction rates and the rate laws. 3) Determine the order of reaction, the rate law, the rate constant, and the rate of concentrations. 4) Solve first-order rate problems.

Rate Mechanisms and Their Structure

Please show all work and keep things as simple as possible in the following three problems on chemistry and its rate mechanisms. The Rate Law. 1) A possible mechanism for the reaction between H2 and CO is shown below, where RDS is the rate-determining step. What is the rate law for the overall reaction? H2 ? 2 H

Chemical Reaction Questions

1. 4CuO(s) + CH4(g) CO2(g) + 4Cu(s) + 2H2O(g) The value of Kc for this reaction is 1.10 at 25.0°C. What is the value of Kp for this reaction? (R = 0.0821 L-atm/K-mol) a. 4.63 b. 26.9 c. 658 d. 37.2 e. 1.52 x 10-3 2. At a certa

Chemical Kinetics: Assessing Reactions

See the attached file. 1. Now consider the following reaction and data: H 2 +2BrCl→2HCl+Br 2 Time (s) Br 2 concentration (M) 5 1.35 15 1.65 Part A What is the average rate of formation of Br 2 ?Express your answer to three decimal places and include the appropriate units. 2. Consider the reaction: A(g)+1 2 B(

Identifying a catalyst in a reaction.

The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below. Identify the catalyst. NO(g)+N2O(g)--->N2(g)+NO2(g) 2NO2(g)-->2NO(g)+O2(g)

Reaction Order

If the overall reaction is the sum of the order of the reagents, and: Zero order = changing concentration of the reactant does not affect the reaction rate. First order = doubling the concentration of any reactant doubles the reaction rate Second order = doubling the concentration of any reactant quadruples the reaction