Question

Please show work and exlpain:

You will need to generate a set of graphs to answer this question.

Concentration vs time data for the following decomposition reaction was collected at 300 K. The data is shown in the table below.

What is the rate constant for the reaction at this temperature (in units of min-1)?

H2O2(aq) → H2O(l) + 1/2 O2(g)

[H2O2](mol/L)	time (min)
0.0200	0
0.0118	500
0.00693	1000
0.00408	1500
0.00240	2000
0.00141	2500

Answer 1

Concepts and reason

Rate law: Rate law is an equation that tells the relation between the rate of the reaction and the concentration of the substrates. The rate constant value can be found using this rate law equation.

Rate law indicates that rate of the reaction is directly proportional to the concentration of the substrates.

Fundamentals

Rate equation for first-order reaction is shown below.

Integrated rate law for the above equation is shown below.

$In[A]=-kt+In[A] $

The above equation represents the straight line.

where,

$slope=-K $

The given balanced reaction is shown below.

The given data are shown below.

[H2O2]	Time (t min)	ln [H2O2]
0.02	0	-3.912023005
0.0118	500	-4.439655748
0.00693	1000	-4.971895466
0.00408	1500	-5.501658291
0.0024	2000	-6.032286542
0.00141	2500	-6.564165575

The graph is shown below between and t.

The graph between ln [A] and time (t) represents a straight line; therefore, the given reaction is a first-order reaction.

Slope of the line from the graph is calculated below.

$slope=-0.0011 $

Ans:

The rate constant for the given reaction is