To predict the rate constant of a reaction graphically using concentration and time data, we can use the following rate equations for different order reactions.
Where
Hence, plotting
yields a straight line with slope -k for zero order reaction.
Plotting
yields a straight line with slope -k for first order reaction.
Plotting
yields a straight line with slope k for second order reaction.
Now, for our given data set, we can plot the above three graphs and determine the order of the reaction and rate constant by whichever plots happen to be a straight line indicating the order.
Hence, the data points we need for the plot are
Now, plotting [H2O2] vs t, we get the following graph.
Note that the graph is not a straight line. Hence, clearly the reaction is not zero order.
Now, we will test for first order kinetics by plotting ln[H2O2] vs. t. Hence, the plot we get is
(1).
Note that the plot is a straight line represented by the fit
equation,
.
Hence, the reaction obeys first order kinetics.
Note: we need not check for the second order kinetics as we found out that the reaction is indeed first order.
We can calculate the rate constant of the reaction from the slope of the graph.
Note that the slope equals negative of the rate constant. Also note that kt is unitless. Hence, unit of the rate constant must be sec-1.
Since the slope is -0.0037, the rate constant of the
reaction is
.
(2).
Now that we know the reaction is first order with respect to H2O2, we can write the following rate law.
Hence, we can calculate the rate of the reaction at
as follows
(3).
The graph of decomposition of H2O2 showing the approximate concentration of H2O2 at t =200 s can be shown as follows:
Hence, the approximate concentration of H2O2 at t=200 s is about 0.42 M.
5. Using the decomposition reaction and the table below, (1) calculate the rate constant of the...
please answer 1 and 2
5. H2O2 decomposition is considered to be first order reaction. Using the table below, 1. Calculate the average rate of reaction 2. Calculate the initial rate of reaction 3. Determine the order of reaction using the integrated rate law equations and using corresponding graphs. Use the instructions on how to enter data and plot a graph on Ti-83/84 Time,s [H202], M 60 120 180 240 300 360 420 480 540 600 0.882 0.697 0.566 0.458...
5) rate = K[A][B] Question 11 (1 point) The reaction mechanism proposed for the decomposition of H202 H2O2 + 12 -> H2O + 10-1 (slow) H2O2 + 10-1 --> H2O + O2 + 12 (fast) Which statement is true? 1) The reaction is second order in 1 2) is an intermediate 3) The reaction is first order in and first order in H2O2. 4) 10 1 is a catalyst. 5) The reaction is zero order in ! Question 12110
Question 3 (Mandatory) (5 points) The rate constant of a first-order decomposition reaction is 0.0147 s. If the initial concentration of reactant is 0.178 M, what is the concentration of reactant after 30.0 seconds? a) 8.72 x 10 M Ob) 0.0785 M Oc) 0,115 M O d) 0.643 M e) 0.0645 M Question 4 (Mandatory) (5 points) The reaction quotient, . for a system is 1.6 x 104. If the equilibrium constant for the system at some temperature 8.5 x...
Table below contains the information on decomposition of ammonia. Using that table calculate the initial and average rate of reaction. Time, min NH3, M 0 6 1 3 2 1.5 3 0.75 4 0.375 5 0.1875 Show your work.
Calculate the rate constant, k, by using Equation
3 (k'=k[OH]^1). Keep in mind, the NaOH solution was
diluted by 50% at the start of the experiment. Write a final
generic rate law using Equation 1 (k[OH]^x[CV]^y)
using the experimental determined values for k, and y. Find the
average for CV (Crystal Violet) order (y), pseudo rate constant
(k'=3.1x10^-8 Ms^-1), and the rate constant (k). The generic rate law is Rate =
k(actual value with correct units)[CV]^(order for cv)[OH]^1.
Section #:...
Calculate the rate constant k (in M^-1 s^-1) using the information
in the reaction and Table 14.2.
ΝΗ, 4 (aq) + NO 2 (aq) →N + 2H2O 2 (8) A) 2.7 x 10*m's' B) 1.0 x 10-ºm's' C) 5.4 x 10m's' D) 2.7 x 10 M's! TABLE 14.2. Rate Data for the Reaction of Ammonium and Nitrite lons in Water at 25 °C + Experiment Number Initial NH, Concentration (M) Initial NO2 Concentration (M) انا فية طالية 0.0100 0.0200 0.0400...
45. Calculate the rate constant k (in M's) using the information in the reaction and Table 14.2 below. Page 8 NH + NO →N + 4 (aq) 2 (aq) 2 (8) 2H 0 (1) A) 2.7 x 10^m's? B) 1.0 x 10PM'sC) 5.4 x 10M's' D) 2.7 x 10-M's! TABLE 14.2 . Rate Data for the Reaction of Ammonium and Nitrite lons in Water at 25 °C Experiment Initial NH, Initial NO2 Observed Initial Number Concentration (M) Concentration (M) Rate...
Using the data in the table, calculate the rate constant of this reaction. Trial[ A(M)[B(M)Rate (M//s)10.3000.3900.017620.3000.8970.093130.4800.3900.0282A+B → C+D
Using the data in the table, calculate the rate constant of this reaction. TrialA(M)B(M)Rate (M//s)10.3000.2600.019920.3000.7280.15630.3900.2600.0259A+B → C +D k = _______
From the data table determine the rate law for reactions 1-4
and calculate the value of k for each. Thanks
I-IV
BACKGROUND
INFORMATION
Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2
Concentration= 0.44 M
•Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M
•Calculation of I^- after mixing for parts I,II, IV= 0.10
M
•Calculation of Initial (mol/L-s)
Filled in Table
Now the solutions for Rate Order and Rate Constant are
needed
Reactants 8 ml 30% HO, 2...